Question

One mole of an ideal gas at atmospheric pressure expands
isobarically from a volume of 1m^{3} to a volume of
2m^{3}.

1 - Find the initial and final temperatures of the gas

2 - Find the work done by the gas

3 - Find the heat added to the gas

Answer #1

(a) For 1 mole of ideal gas the equation of state is

PV = RT

Where, R = 8.314 J/mol.K and we will use

1 atm = 1.01*105 Pa

In initial state, PiVi = RTi

Or, 1.01*105*1 = 8.314*Ti

So, initial temperature, Ti = (1.01*105/8.314) K

= 12148 K

For isobaric system, we can write,

Vi/Vf = Ti/Tf

Or, Tf = (Vf/Vi)*Ti

= {(2*12148)/1} K

Thus, final temperature, Tf = 24296 K

(b) Work done, W = P(Vf - Vi)

= {1.01*105*(2-1)} J

= 1.01*105 J

(c) Heat added, Q = Cp(Tf - Ti)

Where, Cp = specific heat at constant pressure

= 5R/2 = (5*8.314/2) J/mol.K

= 20.785 J/mol.K

So, heat = {20.785*(24296-12148)} J

= 252496.18 J

One
mole of an ideal gas at 25 degrees celsius and one atmosphere
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compresses isothermally back to the original volume, then proceeds
isochorically back to the initial conditions. How much work is done
by the gas?
work done by the ideal gas.

A two mole sample of an ideal diatomic gas expands
slowly and adiabatically from a pressure of 5 atm. and a volume of
10 liters up to a final volume of 30 liters.
a) What is the final pressure of the gas ?,
b) Whatis the heat, work and internal energy?

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A mole of a monatomic ideal gas is taken from an initial
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One mole of a monoatomic, ideal gas at initial pressure
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C) What is the change in heat?
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_____ kJ
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