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Exam 11: Gases and Their Properties

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Question 31

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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 32

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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.

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Question 33

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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?

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?

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.

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

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)

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) ​

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)

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)

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

Absolute zero is the point at which

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?

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)

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

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?

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 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?

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?

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)