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General, Organic And Biochemistry Hybrid Edition 2nd Edition By James Armstrong – Test Bank
Sample Questions
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| Chapter_02_Atoms_Elements_and_Compounds
1. The statement below describes an intensive property.
“The cost of this container of milk is $2.99/gal.”
|
| 2. An element is a shiny gray solid that can be pressed into a thin sheet. This element is probably a metalloid.
|
| 3. Neutral isotopes of the same element have the same number of electrons.
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| 4. The alkali metal found in period 2 is lithium.
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| 5. An isotope of gallium consisting of 31 protons and 37 neutrons can be represented using the symbol shown below.
gallium-37
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| 6. The atomic weight of phosphorus (P) is 30.91 amu or about 31 amu. This indicates that each P atom consists of 15 protons and 16 neutrons.
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| 7. Electron shells define a region in space around the nucleus occupied by certain electrons.
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| 8. The electron arrangement for Na would be:
shell 1: 2 electrons shell 2: 8 electrons shell 3: 1 electron
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| 9. Elements in the same period of the periodic table generally show similar chemical behavior.
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| 10. Group 4A and Group 14 are two different designations for the same column of the periodic table.
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| 11. One of the orbitals in a shell of an atom could be pictured as shown below.
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| 12. An element has the following electron arrangement.
shell 1: 2 electrons shell 2: 8 electrons shell 3: 18 electrons shell 4: 18 electrons shell 5: 7 electrons
The Lewis structure for this element would be:
|
| 13. An elements with an electron arrangement of:
shell 1: 2 electrons shell 2: 8 electrons shell 3: 18 electrons shell 4: 18 electrons shell 5: 7 electrons
would have 1 valence electron.
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| 14. The pie chart shown below represents the elemental composition of the human body including water.
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| 15. The elements sodium, potassium, and oxygen are considered to be “elements of life” and are in the category of electrolytes.
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| 16. A mole of an element contains the same number of atoms as a mole of any other element.
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| 17. In 22.99 g of Na there is 6.022 × 1023 atoms of Na.
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| 18. If the atom ratio of Na to N in a compound is 3:1, the mole ratio of Na to N is 3:1.
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19. When a particular solid sample is examined under a microscope, it is observed that there are regions that are black and regions which are yellow. What type of matter is this sample?
| |
a. |
a compound |
| |
b. |
an element |
| |
c. |
a homogeneous mixture |
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d. |
a heterogeneous mixture |
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20. Sodium is a highly reactive metal and chlorine is a toxic gas, but when they come together the resulting material, sodium chloride (a white solid), is essential for life. Which of the following is true when sodium and chlorine are brought into contact with one another?
| |
a. |
They form a heterogeneous mixture. |
| |
b. |
They form a homogenous mixture |
| |
c. |
They form a new element. |
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d. |
They form a compound. |
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21. Which of the following is a chemical substance than can be broken down into another substance?
| |
a. |
element |
| |
b. |
homogeneous mixture |
| |
c. |
heterogeneous mixture |
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d. |
compound |
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22. Which of the following sequences gives the correct order as we move from left to right across a row of the period table?
| |
a. |
metal, metalloid, nonmetal |
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b. |
metal, nonmetal, metalloid |
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c. |
nonmetal, metal, metalloid |
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d. |
nonmetal, metalloid, metal |
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23. What are the horizontal rows of the periodic table called?
| |
a. |
cycles |
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b. |
periods |
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c. |
groups |
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d. |
columns |
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24. Which of the following groups of elements contains only metals?
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a. |
Ag, As, Ba, Ca |
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b. |
Ag, Au, Pb, Rb |
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c. |
As, Ge, Si, Te |
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d. |
B, Al, Ga, In |
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25. Which subatomic particle(s) are found in the nucleus?
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a. |
only electrons |
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b. |
only neutrons |
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c. |
only protons |
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d. |
both protons and neutrons |
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26. Which of the following correctly describes a proton on a subatomic scale?
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a. |
It is massive and has a +1 charge. |
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b. |
It is massive and has a –1 charge. |
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c. |
It has very small mass and a +1 charge. |
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d. |
It has a very small mass and a –1 charge. |
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| 27. What is the mass number of an atom that is made up of 38 protons, 52 neutrons and 38 electrons?
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28. Which of the following is true of the atomic weight of an element?
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a. |
It is the weight of heaviest isotope. |
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b. |
It is the weight lightest isotope. |
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c. |
It is the weight of the most abundant isotope. |
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d. |
It is an average obtained from the weights and abundances of the isotopes. |
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29. If 1 mol of an element has a mass of 63.54 g, the symbol for this element is
| |
a. |
Eu. |
| |
b. |
Zn. |
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c. |
Cu. |
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d. |
Xe. |
|
| 30. Which of the following is the conversion factor that could be used to convert a mass in grams of sodium to the corresponding number of moles?
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| 31. Which column of the periodic table is commonly called the halogens?
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32. A sealed cylinder is filled with a large collection of atoms that have 14 neutrons and 13 protons. Which of the following would behave in a manner similar to this collection of atoms?
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a. |
a group of atoms with 13 neutrons and 14 protons |
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b. |
a group of atoms with 14 neutrons and 15 protons |
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c. |
a group of atoms with 15 neutrons and 14 protons |
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d. |
a group of atoms with 15 neutrons and 13 protons |
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| 33. Which of the following is the Lewis structure for a nitrogen atom?
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34. What are the elements in the “A” columns of the period table called?
| |
a. |
representative elements |
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b. |
nonmetal elements |
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c. |
metalloid elements |
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d. |
transition elements |
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| 35. Use the periodic table to determine about how many helium atoms (He) on the average would be needed to get close to the same mass as an oxygen atom (O).
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36. Naturally occurring lithium (Li) consists of only two isotopes, Li-6 (6.02 amu) and Li-7 (7.02 amu), where the exact isotopic masses are given in parentheses. Use the periodic table and determine which isotope is present in the larger percentage in the natural element.
| |
a. |
|
| |
b. |
|
| |
c. |
The percentage of each isotope is about the same. |
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d. |
The relative percent abundance cannot be determined from the information available. |
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| 37. How many valence electrons are there in an oxygen atom?
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38. The number of valence electrons of a representative element is related to which of the following?
| |
a. |
atomic number |
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b. |
atomic weight |
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c. |
group number |
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d. |
period number |
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39. How many moles of sulfur are there in a 0.685-g sample of sulfur?
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a. |
0.0214 mol |
| |
b. |
46.8 mol |
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c. |
22.0 mol |
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d. |
32.1 mol |
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| 40. Convert the following number of moles into the corresponding mass.
5.22 mol Br
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a. |
15.3 g |
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b. |
0.0653 g |
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c. |
417 g |
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d. |
79.9 g |
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41. Sodium chlorate, an ingredient in many common herbicides, has sodium, chlorine and oxygen atoms in the ratio 1:1:3, respectively. What is the formula unit for sodium chlorate?
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a. |
NaCO3 |
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b. |
SoClO3 |
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c. |
NaClO3 |
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d. |
none of these |
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42. What is the meaning of the subscripts in the formula for ethyl alcohol, C2H5OH?
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a. |
Each formula unit contains 2 carbon atoms for each oxygen atom. |
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b. |
There are two carbon atoms per formula unit of ethyl alcohol. |
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c. |
Each formula unit contains 3 times as many hydrogen atoms as carbon atoms. |
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d. |
All of these are correct statements. |
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| 43. The image shown below represents an atomic view of a compound CsI.
What is the mass of one formula unit?
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a. |
259.8 g |
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b. |
259.8 amu |
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c. |
1.00 g |
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d. |
6.022 × 1023 amu |
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| 44. Consider the atomic view of a substance shown below.
This substance would be classified as a(n)
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a. |
element |
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b. |
compound |
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c. |
heterogeneous mixture |
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d. |
homogeneous mixture |
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45. Compound consists of five atoms of carbon, ten atoms of hydrogen, and five atoms of oxygen. The formula for this compound is
| |
a. |
CH2O. |
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b. |
C10H5O10. |
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c. |
C5H10O5. |
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d. |
C5H10O10. |
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46. What is the mass of one molecule of glucose, C6H12O6?
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a. |
29.02 amu |
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b. |
180.2 amu |
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c. |
29.02 g |
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d. |
180.2 g |
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47. What is the formula weight of ibuprofen, C13H18O2?
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a. |
29.0 g/mol |
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b. |
206.3 g/mol |
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c. |
289.4 g/mol |
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d. |
377.7 g/mol |
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48. What is the mass of 3.71 mol diethyl ether, C4H10O?
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a. |
20.0 g |
| |
b. |
0.0501 g |
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c. |
74.1 g |
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d. |
275 g |
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49. A person drinks 1900 g of water, H2O, per day. How many moles of water did they consume?
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a. |
mol |
| |
b. |
0.009 mol |
| |
c. |
105 mol |
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d. |
18.02 mol |
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50. If you need a sample of 2.841 mol of Na2S, how many grams do you need?
| |
a. |
0.003640 g |
| |
b. |
2.841 g |
| |
c. |
78.05 g |
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d. |
221.7 g |
|
| 51. How many moles of oxygen would be required to make 4 mol of the following compound?
P4O10
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a. |
40 mol O |
| |
b. |
4 mol O |
| |
c. |
16 mol O |
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d. |
2.5 mol O |
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52. What is the mass of one mole of glucose, C6H12O6?
| |
a. |
29.02 amu |
| |
b. |
180.2 amu |
| |
c. |
29.02 g |
| |
d. |
180.2 g |
|
53. Which of the following is the correct unit for the formula weight of a large number of atoms?
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a. |
amu |
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b. |
g |
| |
c. |
mol |
| |
d. |
molecules |
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| 54. Use the following terms as appropriate to complete the given statement. All terms may not be used.
mass
volume
density
intensive
extensive
The ______________________ of a substance is an example of a ____________________ property.
| ANSWER: |
mass, extensive
volume, extensive
density, intensive |
|
| 55. Use the following terms to complete the two statements given. A term may be used more than once.
heterogeneous mixture
homogeneous mixture
compound
In a restaurant fresh ground pepper is added to olive oil as a dipping sauce for bread. This dip represents a_____________________. Coffee with caramel flavoring is served for dessert. The coffee is an example of a _______________________.
| ANSWER: |
heterogeneous mixture, homogeneous mixture |
|
56. Use one the following terms to complete the given statement.
salt
sugar
vegetable oil
When ____________________ is added to water a heterogeneous mixture forms.
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| 57. Complete the following statement using one of the following terms.
compound
element
mixture
In the manufacture of steel, the percent of manganese is adjusted to determine the brittleness of the product. Steel is an example of a ______________________.
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| 58. Enter the chemical symbol in the blank for the element that has the electron arrangement given below.
shell 1: 2 electrons shell 2: 8 electrons shell 3: 5 electrons
Symbol for the element:_____________________
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| 59. Enter the chemical symbol in the blank for the element described given below.
Representative element in period 4 whose chemical behavior resembles that of O.
Symbol for the element:_____________________
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| 60. Enter the chemical symbol of the element in the blank.
An element has the following electron arrangement.
shell 1: 2 electrons shell 2: 8 electrons shell 3: 18 electrons shell 4: 18 electrons shell 5: 4 electrons
The reactivity of this element would most closely resemble that of which element?
Chemical symbol:_____________________
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| 61. Enter the chemical symbol of the element in the blank.
An element in period 3 has the Lewis structure:
X should be replaced with what chemical symbol?
Chemical symbol:_____________________.
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| 62. Enter the chemical symbol of the element in the blank.
Calcium forms the compound CaF2 . What other alkaline earth element with a smaller atomic mass would form a compound with a similar formula?
Chemical symbol:_____________________.
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| 63. Based on the text periodic table and using the correct number of significant figures, enter the appropriate number in the blank.
The mass of 5.00 mol of oxygen atoms is _____________g.
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| 64. Based on the text periodic table and using the correct number of significant figures, enter the appropriate number in the blank.
The mass of 7.00 mol of sodium chloride, NaCl, is _____________g.
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| 65. Based on the text periodic table and using the correct number of significant figures, enter the appropriate number in the blank.
There are _______mol is 54.05 g of boron.
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| 66. Based on the text periodic table and using the correct number of significant figures, enter the appropriate number in the blank.
There are _______mol is 72.36 g of citric acid, C6H8O7.
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| 67. Enter an integer number (1, 2, 3, …) in the blank.
How many electrons are in shell 2 of a P atom?
____________________electrons
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| Fill in each blank with the appropriate term from the list given below.
protons
neutrons
electrons
valence electrons |
68. N, P and As have the same number of_____________________.
| ANSWER: |
valence electrons |
|
69. and have the same number of _____________________.
| ANSWER: |
protons
electrons |
|
| 70. 14N and 15O have the same number of _____________________.
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| 71. Enter an integer number (1, 2, 3, …) in the blank.
Sucrose (table sugar) has the formula C12H22O11. How many oxygen atoms would be in 3 formula units of sucrose?
____________________oxygen atoms.
| ANSWER: |
33
thirty three
thirty-three |
|
| 72. Enter an integer number (1, 2, 3, …) in the blank.
Sucrose (table sugar) has the formula C12H22O11. A sample of sucrose contains 2400 carbon atoms. How many formula units does this represent?
____________________formula units.
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| 73. Classify the following statement as representing an intensive or extensive property by placing intensive or extensive in the blank.
“Vinegar tastes sour.”: _________________
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| 74. Write the chemical symbol for the elements that is in period 2 and group 8A of the periodic table.
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| 75. Write the name of the following element.
Sn
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| 76. Indicate the number of dots that should be placed around the Lewis symbol for the following element. Use an integer: 1, 2, 3, etc. as appropriate.
Br
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| 77. Convert the following mass moles.
22.98 g glycine, an amino acid, C2H5NO2.
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| Chapter_04_Energy_and_Physical_Properties
1. To convert from joules to kilojoules, move the decimal in the number three places to the right.
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| 2. Butane is a gas at room temperature (25 °C). The boiling point of butane is probably greater than 25 °C.
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| 3. In order to convert a pressure in atmospheres to torr, the following conversion factor should be used.
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| 4. Oxygen, nitrogen and helium are present in a container in which the total pressure is 735 torr. If the pressure of oxygen is 135 torr, that of helium is 55 torr, the pressure of nitrogen is 545 torr.
|
| 5. Diethyl ether historically was used as an anesthetic. Currently, it is a very important solvent. The freezing point and boiling point of diethyl ether are –116 °C and 37 °C, respectively. Diethyl ether is a solid at 0 °C.
|
| 6. Below is the structure of the amino acid, serine. Four hydrogen atoms in the compound can form hydrogen bonds.
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| 7. The two compounds below have the same molecular formula. One would expect A to have a higher boiling point than B.
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| 8. The two compounds below have the same molecular formula. One would expect A to stronger dispersion forces than B.
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| 9. One would expect a compound with the molecular formula C4H10 to have a lower boiling point than one with the formula C7H16.
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| 10. Specific heat is the conversion factor that allows for the calculation of energy based on temperature changes.
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| 11. Either the Kelvin or the Celsius temperature scale can be used in gas law calculations.
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| 12. The following is a mathematical expression of Guy-Lussac’s law.
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| 13. Consider two identical soccer balls. Ball A is kicked and attains a velocity 25 m/sec. Ball B is kicked and attains a velocity of 15 m/sec. At these velocities, Ball A has the greater kinetic energy.
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| 14. Consider a bowling ball with the same diameter and volume as a soccer ball. Both are sitting still on the top of table. Both have the same potential energy.
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| 15. The pressure of a gas is dependent on temperature.
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16. The law of conservation of energy states which of the following?
| |
a. |
Energy cannot be converted from one form to another. |
| |
b. |
Kinetic energy is conserved. |
| |
c. |
Potential energy is conserved. |
| |
d. |
none of the above |
|
17. Which of the following is true as a student slides down a waterslide?
| |
a. |
Their kinetic energy decreases. |
| |
b. |
Their potential energy increases. |
| |
c. |
Their total energy increases. |
| |
d. |
none of the above |
|
18. Which of the following increases as temperature increases?
| |
a. |
kinetic energy |
| |
b. |
attractive forces |
| |
c. |
potential energy |
| |
d. |
none of the above |
|
19. Which of the following is the smallest unit of thermal energy?
| |
a. |
calorie |
| |
b. |
Calorie |
| |
c. |
joule |
| |
d. |
kilojoule |
|
20. The specific heat of ice is 0.480 cal/g°C. How much heat will it take to raise the temperature of 22.50 g of ice from –30.0 °C to –20.0°C?
| |
a. |
108 cal |
| |
b. |
216 cal |
| |
c. |
324 cal |
| |
d. |
469 cal |
|
21. Glycerol changes its shape to conform to its container and has a fairly high density. Glycerol is a:
| |
a. |
solid. |
| |
b. |
liquid. |
| |
c. |
gaseous. |
| |
d. |
either b or c. |
|
22. Which of the following correctly arranges the physical states of matter (gas – g, solid – s, liquid – l) in order of increasing energy of the particles (lowest to highest)?
| |
a. |
g < l < s |
| |
b. |
g < s < l |
| |
c. |
l < g < s |
| |
d. |
s < l < g |
|
23. Which of the following best describes the relationship of molecules in a liquid with those in a gas at the same temperature?
| |
a. |
Molecules in the liquid are much closer together than those in the gas. |
| |
b. |
Molecules in the liquid have less kinetic energy than those in the gas. |
| |
c. |
Molecules in the liquid are moving faster than those in the gas on the average. |
| |
d. |
Both a and b are correct. |
| |
e. |
All of the above are correct. |
|
24. Air pressure can be expressed in which of the following units?
| |
a. |
atmosphere |
| |
b. |
pascal |
| |
c. |
torr |
| |
d. |
any of these |
|
25. Convert 0.662 atm to millibars.
| |
a. |
377 millibar |
| |
b. |
671 millibar |
| |
c. |
millibar |
| |
d. |
0.497 millibar |
|
26. At high altitudes atmospheric pressure is lower than at sea level. Which of the following is true?
| |
a. |
Boiling water is cooler in Denver than in New York. |
| |
b. |
Boiling water is hotter in Denver than in New York. |
| |
c. |
Water boils at the same temperature in Denver and New York. |
| |
d. |
We cannot predict the relationship between the boiling points in the two cities. |
|
27. In which of the following processes does the energy of the water increase?
| |
a. |
water freezes |
| |
b. |
steam condenses to the liquid |
| |
c. |
water evaporates |
| |
d. |
water sublimes |
| |
e. |
both c and d |
|
28. Which of the following phase changes does not involve a solid?
| |
a. |
evaporation |
| |
b. |
melting |
| |
c. |
sublimation |
| |
d. |
freezing |
|
29. On a stove we have two pots of water at the boiling point. Pot 1 contains 1 L of water and pot 2 contains 2 L of water. Which of the following statements is true?
| |
a. |
Pot 2 is at a higher temperature than pot 1. |
| |
b. |
Pot 2 has a larger thermal energy content than pot 1. |
| |
c. |
Both have the same thermal energy content. |
| |
d. |
Both a are b are true. |
|
30. The heat of vaporization of water is 540 cal/g. What mass of water at 100.0 °C can be vaporized by the addition of 55.0 kcal of heat?
| |
a. |
0.19 g |
| |
b. |
55 g |
| |
c. |
g |
| |
d. |
102 g |
|
| 31. Ethylene dichloride is an effective cooling agent when allowed to evaporate. The heat of vaporization is 85.3 cal/g. How much heat could be removed from the skin if 4.25g of ethylene dichloride were sprayed on and allowed to evaporate?
|
32. In which state of matter are the attractive forces between molecules the weakest?
| |
a. |
solid |
| |
b. |
liquid |
| |
c. |
gas |
| |
d. |
None, the attractive forces are about the same in all. |
|
33. Which of the following is the strongest intermolecular attractive force?
| |
a. |
ion-ion attractions |
| |
b. |
dipole-dipole attractions |
| |
c. |
dispersion forces |
| |
d. |
hydrogen bonds |
|
34. Which of the following does not affect the boiling point of a liquid?
| |
a. |
the formula weight of the liquid molecules |
| |
b. |
the shape of the liquid molecules |
| |
c. |
the intermolecular forces between the liquid molecules |
| |
d. |
All of the above affect the boiling point. |
|
35. Which of the following molecules cannot engage in hydrogen bonding?
| |
a. |
CH4 |
| |
b. |
NH3 |
| |
c. |
H2O |
| |
d. |
All of them can hydrogen bond. |
|
36. Which of the following molecules is most likely to be a gas at room temperature?
| |
a. |
PH3 |
| |
b. |
PCl3 |
| |
c. |
PBr3 |
| |
d. |
PI3 |
|
37. Which of the following is a type of heterogeneous mixture?
| |
a. |
suspension |
| |
b. |
solution |
| |
c. |
colloid |
| |
d. |
solvent |
|
38. When alcohol is mixed with water which is the solvent?
| |
a. |
the alcohol |
| |
b. |
the water |
| |
c. |
The substance present in larger amount. |
| |
d. |
The substance present in smaller amount. |
|
| 39. The addition of methanol (CH3OH) to water can be illustrated as shown below.
Based on this image, methanol would be classified as
| |
a. |
an electrolyte. |
| |
b. |
a strong electrolyte. |
| |
c. |
a weak electrolyte. |
| |
d. |
a nonelectrolyte |
| |
e. |
both an electrolyte and a weak electrolyte. |
| |
f. |
both an electrolyte and a strong electrolyte. |
|
40. Potassium phosphate, K3PO4, is a solid at room temperature and is soluble in water. Which of the following statements is correct?
| |
a. |
K3PO4 is an electrolyte. |
| |
b. |
K+ and PO43– ions are solvated by water. |
| |
c. |
K3PO4 completely dissociates in water. |
| |
d. |
All of the above are correct. |
|
| 41. Examine the following representation of a change of state.
Which of the following is the correct term for this change?
| |
a. |
freezing |
| |
b. |
sublimation |
| |
c. |
evaporation |
| |
d. |
boiling |
| |
e. |
melting |
|
42. The use of the energy in food by the body to cause a muscle to contract is an example of
| |
a. |
conversion of heat energy into potential energy. |
| |
b. |
conversion of kinetic energy into potential energy. |
| |
c. |
conversion of potential energy into kinetic energy. |
| |
d. |
conversion of kinetic energy into heal energy. |
|
43. A sample of nitrogen occupies a volume of 543 mL at 30°C and 772 torr. If the temperature is constant, what will be the pressure if the volume changes to 375 mL?
| |
a. |
533 torr |
| |
b. |
torr |
| |
c. |
torr |
| |
d. |
375 torr |
|
44. A balloon with a volume of 5.65 L at room temperature (25°C) is placed in insulated container that is cooled with dry ice where the temperature is –19°C. What is the volume of the balloon in the container when its temperature reaches –19°C? Assume no change in pressure.
| |
a. |
6.63 L |
| |
b. |
4.29 L |
| |
c. |
7.43 L |
| |
d. |
4.82 L |
|
45. A metal gas cylinder is filled with compressed helium at a pressure 2.50 atm when the temperature is 37°C. What is the temperature in Celsius degrees when the pressure in the cylinder changes to 1.78 atm?
| |
a. |
162 °C |
| |
b. |
–52 °C |
| |
c. |
221 °C |
| |
d. |
26 °C |
|
46. An expandable plastic container contains 255 mL of nitrogen gas at 25°C and 688 torr. What is the volume of the container at 47°C and 489 torr?
| |
a. |
385 mL |
| |
b. |
169 mL |
| |
c. |
195 mL |
| |
d. |
334 mL |
| |
e. |
341 mL |
|
47. Air pressure can be expressed in which of the following units?
| |
a. |
atmosphere |
b. |
pascal |
| |
c. |
torr |
d. |
any of these |
|
48. Convert 0.917 atm to millibars.
| |
a. |
697 millibars |
| |
b. |
929 millibars |
| |
c. |
523 millibars |
| |
d. |
1.223 millibars |
|
| Helium (He) is used to fill balloons and is stored in a metal cylinder with pressure gauges on the top.
For each of the following changes, fill the blank with one of the following terms to describe what happens to the pressure reading on the gauge.
increases
decreases
remains constant |
49. Sun shines on the cylinder and warms it, the pressure reading________________________.
| ANSWER: |
increases
Increases |
|
50. Four balloons are filled from the cylinder. The pressure reading _______________________.
| ANSWER: |
decreases
Decreases |
|
51. The cylinder was not secured and fell over, producing a sizable dent in the side. The pressure reading ____________________.
| ANSWER: |
increases
Increases |
|
52. The cylinder was moved from the basement of the building to the fourth floor. The pressure reading _______________________.
| ANSWER: |
remains constant
Remains constant
Remains Constant |
|
53. The 175 g of He was added to the cylinder. The pressure reading ______________________.
| ANSWER: |
increases
Increases |
|
| Filling the blank with the appropriate term from the list below.
Charles’s
Boyle’s
Guy-Lussac’s
Combined Gas |
| 54. The variation in pressure with temperature is defined by ____________________law.
|
| 55. The effect of increasing the temperature on the volume of a gas can be calculated by using _________law.
|
| 56. The following equation is an expression of ______________ law.
|
57. A sample of helium gas is 1.00 atm. If you change the temperature of the sample from 40°C to 110°C and decrease the volume of the container, the resulting pressure can be calculated using ____________________ law.
| ANSWER: |
Combined Gas
combined gas
Combined gas |
|
| In the following sentences, fill in the blanks with the appropriate terms from the list below.
high
low
electrolyte
nonelectrolyte
ion-ion attraction
dipole-dipole attraction
hydrogen bond
dispersion force |
58. _______________________is the type of force present between the particles shown in the image.
| ANSWER: |
Ion-ion attraction
ion-ion attraction |
|
| 59. The melting point of a solid composed of the particles shown in the image will be _________________.
|
| 60. This substance is water-soluble. A solution of this compound in water would be classified as a(n)_______________________.
|
| 61. The boiling point of the substance shown below will be ______________________ when compared to that of substance in the image.
.
|
| Consider the image given below of a pair of ammonia molecules. Complete the following sentences using the appropriate terms listed below.
covalent bond
hydrogen bond
ion-dipole attraction
donor
acceptor |
62. Each solid line in the figure represents a_______________________.
| ANSWER: |
covalent bond
Covalent bond
Covalent Bond |
|
63. The dashed line in the figure represents a__________________.
| ANSWER: |
hydrogen bond
Hydrogen bond
Hydrogen Bond |
|
| 64. The nitrogen atom in the lower right ammonia molecule is a hydrogen bond _____________________.
|
| 65. The lower middle hydrogen atom in the upper left ammonia molecule could be a hydrogen bond _____________________.
|
| Consider the following three substances.
A B C
Enter the letter of the appropriate substance in the blank provided. If none applies, enter the word none. |
| 66. The substance capable of hydrogen bonding is _____.
|
| 67. Substance(s) that _____ is(are) soluble in water.
|
| 68. Substance _____ would form a heterogeneous mixture with water.
|
| 69. Substance____can function as a hydrogen bond acceptor but not a hydrogen bond donor.
|
70. When you inhale and exhale does your rib cage raise or lower? Why?
| ANSWER: |
Upon inhalation, the rib cage raises to make room for the lungs to expand (increases volume which momentarily decreases pressure), in order to receive O2. Air flows in to equalize the pressures. Upon exhalation, the rib cage lowers (decreases volume which momentarily increases pressure) to push air (containing CO2) out of the lungs. Air flows out to equalize the pressures. |
|
| 71. A convenient reference set of conditions for gases is STP (Standard Temperature and Pressure). There conditions are defined as exactly 0°C and 1.00 atm. If a sample of a gas have a volume of 2.57 L at a temperature of 27°C and 1.25 atm. What is the volume of this gas at STP?
|
| 72. The volume of a gas in the upper atmosphere needs to be calculated. If the temperature is –41°C, what numerical value should be used in the calculation?
|
| 73. What is the specific heat of a substance if it requires 475 cal to raise the temperature of a 67-gram sample from 25°C to 43°C?
|
| 74. A gas cylinder contains three gases: oxygen, nitrogen, and helium. The partial pressure of oxygen is 4.7 psi and the partial pressure of nitrogen is 3.0 psi. If the reading on the pressure gauge is as shown below.
What is the partial pressure of the He?
|
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