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Exam 5: Gases

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Question 31

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A sample of a gas occupies 1.40 * 10³ mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?

A) 2,800 mL
B) 2,100 mL
C) 1,400 mL
D) 1,050 mL
E) 700 mL

F) All of the above
G) B) and D)

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Question 32

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What is the pressure (in atmospheres)of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 735 mmHg and h = 8.3 cm?

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Question 33

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The van der Waals equation is a modification of the ideal gas equation. For what two facts does this equation account?

Calculate the volume occupied by 25.2 g of CO₂ at 0.84 atm and 25°C. R = 0.08206 L.atm/K.mol.

How many molecules of N₂ gas can be present in a 2.5 L flask at 50°C and 650 mmHg?

At constant pressure, the density of a gas depends on temperature. Does the density increase or decrease as the temperature increases?

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm. If the can contains 1.0 g CO₂ and is heated to 400°C, will it burst?

A mixture of three gases has a total pressure of 1,380 mmHg at 298 K. The mixture is analyzed and is found to contain 1.27 mol CO₂, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of Ar?

Calculate the number of moles of gas contained in a 10.0 L tank at 22°C and 105 atm. (R = 0.08206 L.atm/K.mol)

What is V in the table below?

A 1.07 g sample of a Noble gas occupies a volume of 363 mL at 35°C and 678 mmHg. Identify the Noble gas in this sample? (R = 0.08206 L.atm/K.mol)

A sample of carbon monoxide gas was collected in a 2.0 L flask by displacing water at 28°C and 810 mmHg. Calculate the number of CO molecules in the flask. The vapor pressure of water at 28°C is 28.3 mmHg.

What is the pressure of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 736 mmHg and h = 9.2 cm?

A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at -4.0°C. Which of these choices is its molecular formula?

A 0.271 g sample of an unknown vapor occupies 294 mL at 140°C and 847 mmHg. The empirical formula of the compound is CH₂. What is the molecular formula of the compound?

What is standard temperature and standard pressure?

The pressure of a gas sample was measured to be 489 mmHg. Which of the following is not an equivalent statement of that pressure? (1 atm = 1.01325 * 10⁵ Pa)

A small bubble rises from the bottom of a lake, where the temperature and pressure are 4°C and 3.0 atm, to the water's surface, where the temperature is 25°C and the pressure is 0.95 atm. Calculate the final volume of the bubble if its initial volume was 2.1 mL.

Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be exerted by 2,500 g of oxygen gas (O₂) when stored at 22°C in a 40.0 L cylinder?

A sample of mercury(II) oxide is placed in a 5.00 L evacuated container and heated until it decomposes entirely to mercury metal and oxygen gas. The container is then cooled to 25°C. One now finds that the gas pressure inside the container is 1.73 atm. What mass of mercury(II) oxide was originally placed into the container?