Chem 1010 - General Chemistry 1 » Summer 2022 » Quiz 7

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Question #1
One atmosphere of pressure is equal to 760 mmHg. This unit is used in the common barometer and manometer. Determine height (in mm) of a column of liquid bromine if the pressure is one atmosphere. The densities of mercury and bromine are 13.546 and 3.119 g/cm3, respectively
A.   4.34
B.   1.75 × 102
C.   3.30 × 103
D.   0.00571
Question #2
One atmosphere of pressure is equal to 760 mm Hg. This unit is used in the common barometer and manometer. Determine the height (in mm) of a column of ethanol if the pressure is 0.955 atmosphere. The densities of mercury and ethanol are 13.546 g/cm3 and 0.79 g/cm3, respectively.
A.   42
B.   1.2 × 104
C.   46
D.   1.4 × 104
Question #3
The firmness of a balloon can be used to explain that:
A.   many of the gases we breathe are diatomic
B.   gases inside the balloon exert pressure
C.   air is a mixture of molecular compounds
D.   gases can be compressed into liquids
Question #4
Which concept is not associated with the kinetic-molecular theory of gases?
A.   The average kinetic energy of gas molecules increases as the temperature increases.
B.   No energy is lost when gas molecules collide with each other
C.   The forces of attraction and repulsion between separate gas molecules are minimal
D.   The velocity of a gas molecule is inversely proportional to its temperature.
Question #5
Which description of the kinetic-molecular theory of gases is true?
A.   Gas molecules move randomly in all directions with the same speed.
B.   The forces of attraction and repulsion do not exist for gas molecules
C.   The space between two gas molecules is much greater than the size of each gas molecule
D.   Colliding gas molecules have the same speed before and after the collision.
Question #6
What happens to a helium balloon at a party on a hot day if the balloon was filled on a cold morning?
A.   The balloon shrinks because the warmer day temperature causes the helium atoms to be more attracted to each other and allows them to occupy less space inside the balloon.
B.   The balloon shrinks because the warmer day temperature speeds up the helium atoms and increases the number of atoms that escape through the inner wall of the balloon.
C.   The balloon expands because the warmer day temperature causes the helium atoms to be less attracted to each other and allows them to occupy more space inside the balloon.
D.   The balloon expands because the warmer day temperature speeds up the helium atoms and increases the force and frequency of gas collisions on the inner wall of the balloon.
Question #7
If, at constant temperature, the pressure of a flask equipped with a moveable piston is increased to 3 times its original pressure, what must happen to the volume?
A.   No change in volume occurs.
B.   The volume increases to 3 times the original volume
C.   The volume decreases to 1/9 the original volume.
D.   The volume decreases to 1/3 the original volume.
Question #8
Which statement about ideal gases and the gas laws is false?
A.   The laws describe the macroscopic behavior of ideal gases.
B.   The laws are summarized as equations that describe the behavior of ideal gases.
C.   A gas will behave ideally under all conditions.
D.   Variables that appear in the laws are temperature, pressure, volume, and amount of gas.
Question #9
If a 2.0-liter sample of gas experiences a decrease in pressure from 1.74 atm to 0.555 atm at 25°C, what is the resulting volume (in L) at 25°C?
A.   20 L
B.   0.64 L
C.   0.48 L
D.   6.3 L
Question #10
At 20°C, a sample of gas has a volume of 2.51 L at 795 torr. What is the new pressure (in atm) if the volume is increased to 6.46 L at the same temperature?
A.   2.69
B.   0.813
C.   309
D.   0.406

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