Question

A 0.505-mol sample of an ideal diatomic gas at 408 kPa and 309 K expands quasi-statically until the pressure decreases to 150 kPa. Find the final temperature and volume of the gas, the work done by the gas, and the heat absorbed by the gas if the expansion is the following.

(a) isothermal

final temperature K

volume of the gas

L

work done by the gas

J

heat absorbed

J

(b) adiabatic

final temperature K

volume of the gas L

work done by the gas J

heat absorbed J

Answer #1

2.50 mol of a diatomic ideal gas expands adiabatically and
quasi-statically. The initial temperature of the gas is 325 K. The
work done by the gas during expansion is 7.50 kJ.
(a) What is the final temperature of the gas?
K
(b) Compare your result to the result you would get if the gas
were monatomic. (Calculate the final temperature if the gas were
monatomic.)
K

Suppose 4.00 mol of an ideal gas undergoes a reversible
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A two mole sample of an ideal diatomic gas expands
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A vessel with a movable piston contains 1.90 mol of an ideal gas
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Pi = 2.03 ✕ 105 Pa,
initial volume
Vi = 1.00 ✕ 10−2
m3,
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J
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A sample consisting of 2.5 moles of ideal gas (Cp,m
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Calculate the final volume, the final temperature, and the work
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A 2.0 mol sample of ideal gas with molar specific heat
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ir is mostly a mixture of diatomic oxygen and nitrogen; treat it
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Theuniversalgasconstantis?=8.315J⋅mol−1 K−1. The compression
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