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Exam 11: Gases and Their Properties

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Question 31

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It is possible to make a barometer using a liquid other than mercury. What would be the height (in meters) of a column of dichloromethane at a pressure of 0.790 atm, given that 0.790 atm is equal to a 0.600 m column of mercury and the densities of mercury and dichloromethane are 13.5 g/cm³ and 1.33 g/cm³, respectively.

A) 6.09 m
B) 0.164 m
C) 0.0592 m
D) 0.799 m
E) 1.25 m

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Question 32

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A balloon is filled with He gas to a volume of 2.10 L at 35 °C. The balloon is placed in liquid nitrogen until its temperature reaches -196 °C. Assuming the pressure remains constant, what is the volume of the cooled balloon?

A) −0.375 L
B) 0.375 L
C) 0.525 L
D) 0.00909 L
E) 8.40 L

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Question 33

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Which of the following samples contains the fewest moles of gas?

A particular gas exerts a pressure of 5.35 × 10⁴ Pa. What is this pressure in units of atmospheres? (1 atm = 760 mm Hg = 101.3 kPa = 1.013 bar) ​

A sample of helium gas occupies 17.9 L at 23°C and 0.956 atm. What volume will it occupy at 40°C and 1.20 atm?

The density of a gas is 1.25 g/L at STP. What is its molar mass?

What volume of O₂, measured at 24.0°C and 0.882 atm atm, will be produced by the decomposition of 3.00 g KClO₃? Assume 100% yield. (R = 0.08206 L?atm/mol?K) 2 KClO₃(s) ? 2 KCl(s) + 3 O₂(g)

A gas sample is heated from −20.0°C to 57.0°C and the volume is increased from 2.00 L to 4.50 L. If the initial pressure is 0.150 atm, what is the final pressure?

The ideal gas law can be modified to correct for the errors arising from nonideality. The modified equation is known as the ________ equation of state for a real gas.

A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6°C. Determine the temperature at which the volume of the gas is 3.47 L.

Sodium azide decomposes rapidly to produce nitrogen gas. 2 NaN₃(s) → 2 Na(s) + 3 N₂(g) What mass of sodium azide will inflate a 60.0 L airbag for a car to a pressure of 1.50 atm at 32 °C? (R = 0.08206 L⋅atm/mol⋅K)

Absolute zero is the point at which

The density of ethane, C₂H₆ (30.1 g/mol) , at 27°C and 1.27 atm pressure is ___. (R = 0.08206 L⋅atm/mol⋅K)

Gaseous chlorine is held in two separate containers at identical temperatures and pressures. The volume of container 1 is 1.30 L, and it contains 6.70 mol of the gas. The volume of container 2 is 2.75 L. How many moles of the gas are in container 2?

One way to isolate metals from their ores is by a chemical reaction of the metal oxide with carbon as shown below (M = metal) : $2 \mathrm { MO } ( s ) + \mathrm { C } ( s ) \rightarrow 2 \mathrm { M } ( s ) + \mathrm { CO } _ { 2 } ( g )$ If 31.75 g of a metal oxide reacts with excess carbon to form 4.07 L of CO₂ at 100°C and 1.50 atm, what is the identity of the metal?

What volume of oxygen will react with 21 mL of ethanol, assuming the gases are present at the same temperature and pressure? 2 CH₃CH₂OH(g) + 6 O₂(g) → 4 CO₂(g) + 6 H₂O(g)

When 0.5000 grams of an unknown hydrocarbon, C_xH_y, is completely combusted with excess oxygen, 1.037 L CO₂ gas and is produced at 98.3 °C and 1.000 atm. What is the empirical formula of the hydrocarbon? (R = 0.08206 L⋅atm/mol⋅K)

A flexible vessel contains 53 L of gas where the pressure is 1.1 atm. What will the volume be when the gas is compressed to a pressure of 0.91 atm, the temperature remaining constant?

The gas constant, R, expressed in SI units has a value of 8.314. The units of the constant are ________.

Carbon monoxide reacts with oxygen to form carbon dioxide. 2 CO(g) + O₂(g) → 2 CO₂(g) In a 1.00 L flask, 4.30 atm of CO reacts with 2.50 atm of O₂. Assuming that the temperature remains constant, what is the final pressure in the flask?