 |
1 | |
Convert .573atm to torr. |
| | A) | 43.5torr |
| | B) | 435.48torr |
| | C) | 4.35torr |
| | D) | 499torr |
| | E) | None of the above |
|
|
2 | |
A bicycle tire at a certain temperature exhibits a pressure of 437torr and occupies a volume of 13.2L. Calculate the pressure in atm if the volume is decrease to 5.9L. |
| | A) | 1.29atm |
| | B) | 699atm |
| | C) | 12.9atm |
| | D) | .950atm |
| | E) | 32.2atm |
|
|
3 | |
Which of the following is a correct statement of Boyle's Law? |
| | A) | P/T = constant |
| | B) | V/P = constant |
| | C) | V x P = constant |
| | D) | T/V = constant |
| | E) | V/T = constant |
|
|
4 | |
27.5 grams of gas at 2.00atm is compressed from 9.00L to 5.00L at constant temperature. What is the final pressure in atm? |
| | A) | 3.60atm |
| | B) | 2.00atm |
| | C) | 45.0atm |
| | D) | 1.11atm |
| | E) | 4.00atm |
|
|
5 | |
23 x 1023 molecules of a gas at 3.50atm is expanded at constant temperature from 9.00L to 15.00L. What is the final pressure in atm? |
| | A) | 5.83atm |
| | B) | 3.58atm |
| | C) | 3.50atm |
| | D) | 2.10atm |
| | E) | 58.3atm |
|
|
6 | |
What is the new volume of an unknown gas if it was originally at 37oC and 1.00atm in a 5.90L tank, and it is cooled at unchanging pressure until the temperature is 13oC? |
| | A) | 2.07L |
| | B) | 16.7L |
| | C) | 81.5L |
| | D) | 5.44L |
| | E) | 7.02L |
|
|
7 | |
A large natural gas storage tank was made so that the pressure is maintained at 3.25atm. On a hot day, when the temperature is 42.0oC, the volume of gas in the tank is 29,325ft3. What is the volume of the same quantity of gas on a cold day of -17oC? |
| | A) | 2.38 x 104 ft3 |
| | B) | 2.40 x 104 ft3 |
| | C) | -7.29 x 104 ft3 |
| | D) | 1.20 x 104 ft3 |
| | E) | -3.63 x 104 ft3 |
|
|
8 | |
1.00 mole of nitrogen gas is confined at room temperature at 22.0oC. What is the volume of this gas under a pressure of 1.00atm? |
| | A) | 24.2L |
| | B) | 22.2L |
| | C) | 23.2L |
| | D) | 22.0L |
| | E) | 42.2L |
|
|
9 | |
What is the density of O2 gas at STP? |
| | A) | 1.43g/L |
| | B) | 4.17g/L |
| | C) | 22.4g/L |
| | D) | 16.0g/L |
|
|
10 | |
What is the density of CH4 gas vapor at 714torr and 125oC? |
| | A) | 4.60g/L |
| | B) | 16.0g/L |
| | C) | 714g/L |
| | D) | 0.460g/L |
| | E) | 71.4g/L |
|
|
11 | |
A sample of carbon dioxide (CO2) gas occupies 5.00L at 27oC and at 1.00atm. What is its new volume if the temperature and pressure are 48.0oC and 1.70atm? |
| | A) | 5.00L |
| | B) | 8.50L |
| | C) | 4.80L |
| | D) | 3.15L |
| | E) | 1.70L |
|
|
12 | |
Oxygen gas (O2) reacts with methane gas (CH4) during its combustion to form carbon dioxide and water. What volume of CH4 (g) at 725mmHg and at 21.5oC is required to react with 9.35L of O2 (g) at the same temperature and pressure? |
| | A) | 7.25L |
| | B) | 9.35L |
| | C) | 21.5L |
| | D) | 46.8L |
| | E) | 4.68L |
|
|
13 | |
How many molecules of CO2 (g) are contained in 1.25mL at STP? |
| | A) | 6.02 x 1023 molecules |
| | B) | - 6.02 x 1023 molecules |
| | C) | 6.02 x 1019 molecules |
| | D) | 3.36 x 1019 molecules |
| | E) | 1.25 x 1023 molecules |
|
|
14 | |
Calculate the molar mass of a gas if its density is 2.52g/L at STP conditions. |
| | A) | 2.52g/mole |
| | B) | 25.2g/mole |
| | C) | 252g/mole |
| | D) | 56.4g/mole |
| | E) | 8.25g/mole |
|
|
15 | |
17.5L of gas is heated from 29.0oC to 71.0oC at constant-pressure conditions. Under these conditions, which of the following statements is true? |
| | A) | The number of moles of gas increases. |
| | B) | The number of moles of gas decreases. |
| | C) | The volume decreases. |
| | D) | The volume increases. |
| | E) | The temperature is constant. |
|
|
16 | |
Which of the following statements about the properties of a gas are correct when the pressure decreases at an unchanging temperature? |
| | A) | Volume decreases. |
| | B) | The ideality of gas changes. |
| | C) | The average molecular speed of a gas decreases. |
| | D) | The average molecular speed of a gas increases. |
| | E) | Volume increases. |
|
|
17 | |
A glass bulb was filled with the vapors of volatile liquid at 150oC, and at 785torr. The net weight for the sample in the bulb under these conditions was .119g. When the bulb was filled with water at 25oC, the volume of the bulb was found to be 125mL. Calculate the molar mass of the unknown gas. |
| | A) | 0.785g/mole |
| | B) | 0.250g/mole |
| | C) | 44.0g/mole |
| | D) | 32.0g/mole |
| | E) | 98.0g/mole |
|
|
18 | |
The metabolic breakdown of glucose, C6H12O6, in our bodies produces CO2 gas as follows: C6H12O6 (s) + 6O2 (g) --> 6CO2 (g) + 6H2O (l) Calculate the volume of dry CO2 gas produced at 37oC and 1.00atm when 7.50g of glucose is consumed in this reaction. |
| | A) | 7.50L |
| | B) | 191L |
| | C) | 6.36L |
| | D) | 3.71L |
| | E) | 4.56L |
|
|
19 | |
Ammonium sulfate, an important fertilizer, can be prepared by the reaction of ammonia with sulfuric acid: 2NH3 (g) + H2SO4 (aq) --> (NH3)2SO4 (aq) Calculate the volume of NH3 gas needed at 25.00oC and 27.00atm to react with 135.0kg of H2SO4 (aq). |
| | A) | 209.4L |
| | B) | 2497L |
| | C) | 2094L |
| | D) | 10.26L |
| | E) | 1026L |
|
|
20 | |
Which of the following statements describes pressure at the molecular level? |
| | A) | Pressure is caused by molecules colliding with each other. |
| | B) | Pressure is caused by molecules being pulled down by gravity. |
| | C) | Pressure is caused by molecules colliding with their container. |
| | D) | Pressure is caused by molecules moving faster when more molecules are added. |
| | E) | Pressure is caused by molecules gaining mass due to their high velocity. |
|