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AP Chemistry > Chapter 5 Review > Flashcards

Chapter 5 Review Flashcards

1
Q

In a chemical reaction, a gas has a final pressure of 1.37 atm. What is the equivalent pressure in units of torr?

A

1,040 torr

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2
Q

A manometer shows a mercury level of 225 mm Hg on the closed end of the tube and 108 mm Hg on the open end. If the atmospheric pressure is 760 torr, what is the pressure of the gas (in mm Hg or torr) in the closed end of the manometer?

A

643 torr

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3
Q

If a gas exerts pressure of 2.25 atm, what is its pressure in millimeters of mercury?

A

1710 mm Hg

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4
Q

What will happen to the volume of a gas if the pressure is decreased? Assume that the amount of gas and the temperature remain constant.

A

The volume will increase

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5
Q

Suppose you are holding a balloon that contains 28 L of air at a standard atmospheric pressure of 14.7 lb / in2. If you squeezed the balloon until the pressure inside was 55 lb / in2, what would the final volume of the squeezed balloon be? Assume that the temperature remains constant.

A

7.5 L

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6
Q

Using Boyle’s Law, predict what will happen to the volume of a gas if there is an increase in pressure. Assume that the temperature and the number of moles of gas remain constant.

A

The volume will decrease.

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7
Q

Suppose you fill a balloon with 23 L of gas at an atmospheric pressure of 1.0 atm. What will the new volume of the balloon be if you place it in an area that has an atmospheric pressure of 0.45 atm?

A

51 L

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8
Q

According to Charles’s Law, what will happen to the temperature of a gas if the volume is decreased (while the gas remains at a constant pressure)?

A

The temperature will decrease.

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9
Q

At what temperature (Kelvin) would a gas have no volume at all?

A

0 K

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10
Q

Suppose that 2.3 L of gas at 35°C and 1.0 atm is expanded to 4.5 L at 42°C. What will the final pressure of the gas be?

A

0.52 atm

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11
Q

Suppose you have a sample of gas. You simultaneously decrease the volume and raise the temperature. What happens to the pressure?

A

the pressure goes up

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12
Q

Suppose that a 4.0 L sample of gas at 1.0 atm is heated from 44°C to 53°C, and during this process the volume doubles. What will the final pressure of the gas sample be?

A

0.51 atm

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13
Q

The Combined Gas Law states that (PiVi / Ti ) = (PfVf  / Tf ). Which statement best explains how this law also includes Boyle’s Law?

A

When the temperature is constant, the pressure and volume are inversely proportional.

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14
Q

A helium balloon at 25°C, 1 atm, has a volume of 2.88 L. Additional helium is pumped into the balloon. It now contains 1.20 g of He and its new volume is 7.20 L. How many moles of helium gas did the balloon contain originally?

A

0.12 mol

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15
Q

What empirical gas law is illustrated when inflating a balloon?

A

Avogadro’s law

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16
Q

A helium balloon contains 0.10 mol of gas and has a volume of 2.4 L (at 25°C, 1 atm). We inflate the balloon by adding 0.13 mol of helium. What is the new volume of the balloon?

A

5.5 L

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17
Q

Calculate the pressure of 0.800 moles of helium gas, when the gas is in a balloon with a volume of 2.30 L at a temperature of 32°C.

A

8.71 atm

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18
Q

A poisonous gas is being transported from Texas to California. The container is 4000.0 L and 4°C. It can withstand a pressure of 100.0 atm. Which of the following is the maximum safe amount of gas to ship?

A

1.76 × 10^4 mol

19
Q

What is the pressure exerted by 4.5 mol of a gas in a 15.0 L flask at 285 K?

A

7.0 atm

20
Q

The density of a gas at standard temperature is 2.30 g / L. What is the pressure of 1.00 mole of the gas if there are 0.00446 kg of gas present?

A

11.5 atm

21
Q

There is an unlabeled gas cylinder in the chemistry lab. The cylinder contains a gaseous compound. A sample of the compound shows that it contains 27.27% carbon and 72.73% oxygen. The 1.50 L bottle was found at STP and contained 2.94 g of the compound. Identify the number of moles of the compound in the bottle.

A

0.0669 mol

22
Q

Two gas tanks are linked by a connecting tube with a valve. One contains 10 L of helium at 6.7 atm of pressure. The other contains 4.2 L of nitrogen at 3.6 atm of pressure. If the valve is opened, what is the final pressure of the two tanks combined?

A

5.8 atm

23
Q

A tank of gas is found in the coldest part of the refrigerator (at “standard temperature,” 0°C = 273 K). It contains 4 moles of gas: 1 mole of oxygen and 3 moles of neon. The volume of the tank is 11.2 L. What is the partial pressure of oxygen in the tank?

A

2.0 atm

24
Q

What does the mole fraction of a gas in a tank which contains a mixture of gases equal?

A

It is equal to the ratio of the number of moles of a particular gas to the total number of moles of gas in the tank.

25
Q

Two gas tanks are linked by a connecting tube with a valve. This time, one contains 6.5 L of oxygen at 5.4 atm of pressure. The other contains 9.0 L of argon at 3.7 atm of pressure. If the valve is opened, what is the final pressure of the two tanks combined?

A

4.4 atm

26
Q

The Haber-Bosch process is used industrially to produce ammonia (NH3 ) from nitrogen and hydrogen through the reaction
N2(g) + 3H2(g) → 2NH3(g)
After running the process in a 612 L tank at 559°C for three hours, 242 moles of ammonia have been produced and 128 moles of H2 remain. If the initial total pressure of the system was 127.7 atm, what was the initial partial pressure of N2?

A

72.9 atm

27
Q

A sample of hydrogen gas is collected over water. We measure the temperature, pressure, and volume, and use our knowledge of the gas law to calculate that the sample contains 1.43 × 10−3 moles of hydrogen. What is the mass of the hydrogen collected?

A

2.88 mg

28
Q

Which of the following statements best describes the vapor pressure of water?

A
  • It depends on the temperature of the water only.

- It is always a component of the total pressure when a gas is collected over water

29
Q

Identify the staement which best explains why a hot air balloon rises.

A

The density of hot air is less than the density of cold air.

30
Q

On a nice summer day on a mountain top, the temperature is 29.0°C and the air pressure is 700.0 torr. What is the volume of 1.0 mole of gas? (R = 0.08206 L • atm / mol • K)

A

27 L

31
Q

What is the density of methane gas, CH4, at STP?

A

0.714 g / L

32
Q

in our lecture, the formula P NMu^2/V was converted to the ideal gas formula, PV=nRT, by using which formula

A

mu^2 - T

33
Q

Is the following statement true or false? The kinetic molecular theory of gases links observations at a macroscopic level (such as pressure and temperature) to an explanation of what is happening at a molecular level (with regard to velocity, mass and number of collisions).

A

True

34
Q

A tightly sealed oxygen cylinder is taken from an air-conditioned building and left in a hot car in a parking lot. What happens to the average kinetic energy and the pressure of the oxygen molecules?

A

Kinetic energy and pressure both increase.

35
Q

What is the root mean square speed of methane, CH4, at 25°C?

A

681 m / sec

36
Q

Study the graph. Which of the following statements is not true about O2?

A

O2 has more molecules at higher speeds than helium.

37
Q

Which of the following statements about the graph is not correct?

A

The mass of a nitrogen particle must be larger than the mass of an oxygen particle at a given temperature.

38
Q

Which of the following statements referring to the graph is true?

A

O2 particles at 25°C have a smaller range of distribution than O2 particles at 1000°C.

39
Q

The ratio of the rate of effusion of gas 2 to the rate of effusion of gas 1 is 0.22. If the molar mass of gas 1 (Mgas 1 ) is 3.79 g / mol, what is the molar mass of gas 2?

A

78 g / mol

40
Q

Which of the following best defines effusion?

A

Effusion is the movement of gas particles through a pinhole into a vacuum.

41
Q

The molar mass of gas 1 is 5.08 g / mol. If the rate of effusion of gas 1 is 3.57 times faster than the rate of effusion of gas 2, what is the molar mass of gas 2?

A

64.7 g / mol

42
Q

Consider 5.0 moles of O2 in a 2.0 liter container at 300.0 K. What is the pressure calculated by the van der Waals equation of state minus the pressure predicted by the ideal gas law? The ideal gas law constant is 0.08206 [L•atm] / [mol•K]. For O2, the pressure correction constant is 1.382 [L2•atm] / [mol 2 ], and the volume correction constant is 0.03186 L / mol.

A

−4 atm

43
Q

Under which condition does the behavior of a real gas approach the behavior of an ideal gas?

A

as the pressure approaches 0 atm

44
Q

At low pressures, why is the compressibility factor of real gases often lower than that of an ideal gas?

A

Attractive intermolecular interactions decrease the space between real gas molecules.

AP Chemistry (338 decks)

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