If the heat capacity of a diatomic IDEAL gas is 29.0 J/k mol, calculate what the

Question

If the heat capacity of a diatomic IDEAL gas is 29.0 J/k mol, calculate what the change in entropy is for one mol of ideal gas if it is heated from 100K ? 200K, and also from 100K ? 1000K at constant P.

2. An ideal gas assumes molecules are point particles and do not interact with each other. In reality, molecules occupy space! To correct for this, the ideal gas equation of state is adjusted to take the volume occupied by the molecules into account for a real gas PV nRT or P = nRTN is modified to P = nRT/(V-nb) (IDEAL GAS) (REAL GAS) comparison to propane. Consider a value of "b"~ 4x10-5 m3 /mol, which is average for small diatomic and triatomic molecules

Explanation / Answer

For an ideal gas, change of entropy at constant pressure

dS = n.Cp.ln(T2/T1)

= 1 mol*(29.0 J/k mol)*ln(200/100)

= 20.101 J/K

When heated from 100K to 1000K,

dS = n.Cp.ln(T2/T1)

= 1 mol*(29.0 J/k mol)*ln(1000/100)

= 66.775 J/K

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