A cylinder of volume 0.260 m3 contains 11.2 mol of neon gas at 22.4°C. Assume neon behaves as an ideal gas. (a) What is the pressure of the gas?  Pa (b) Find the internal energy of the gas.  J (c) Suppose the gas expands at constant pressure to a volume of 1.000 m3. How much work is done on the gas? J

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A cylinder of volume 0.260 m3 contains 11.2 mol of neon gas at 22.4°C. Assume neon behaves as an ideal gas.

(a) What is the pressure of the gas?
 Pa

(b) Find the internal energy of the gas.
 J

(c) Suppose the gas expands at constant pressure to a volume of 1.000 m3. How much work is done on the gas?
J

(d) What is the temperature of the gas at the new volume?
Expert Solution
Step 1

As the gas behaves like an ideal gas, the ideal gas equation is

PV=nRTP is the pressure of gasV is the volume of gasn is the no of moles of the gasR is the gas constantT is the temerature of te gas

P=nRTVThe volume of the gas is equal to the volume of the containerV=0.26 m3R is the gas constant=8.314 J/K molT=22.4°C=22.4+273=295.4°KP=11.2×8.314×295.40.26P=1.058×105 Pa

Step 2

As the gas is stored in a 3-d container, the gas molecules have namely 3 degrees of freedom, i.e. along the x, y, and z axes.

The internal energy of such a gas is given as

U=D.O.F2nRTU=32nRTU=32×11.2×8.314×295.4U=4.126×104 J

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