Imagine 1.63 moles of NH3(g) undergo reversible, adiabatic expansion from 1.6 L to 5.6  L at 333 K. The molar heat capacity at constant volume of NH3(g) is 28.05 J/molK at 333  K. You may assume perfect gas behavior. Calculate the work done.

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Imagine 1.63 moles of NH3(g) undergo reversible, adiabatic expansion from 1.6 L to 5.6 
L at 333 K. The molar heat capacity at constant volume of NH3(g) is 28.05 J/molK at 333 
K. You may assume perfect gas behavior. Calculate the work done.

Expert Solution
Step 1: Adiabatic process

For adiabatic process 

bold italic T subscript bold 1 bold V subscript bold 1 to the power of bold gamma bold minus bold 1 end exponent bold equals bold italic T subscript bold 2 bold V subscript bold 2 to the power of bold gamma bold minus bold 1 end exponent----------- eq (1)

where,

T1 = initial temperature,

T2 = final temperature,

V1 = initial volume

V2 = final volume

bold italic gamma bold equals bold c subscript bold p over bold c subscript bold v ----------eq (2)

where,

cp = heat capacity at constant pressure,

cv = heat capacity at constant volume

Relation between cp and cv   (for an ideal gas)

bold italic c subscript bold p bold minus bold italic c subscript bold v bold equals bold italic R ----------- eq(3)

where R is unversal gas constant ( 8.314 J K-1mol-1)

Work can be calculated for and adiabatic reversible process from equation,

bold italic w bold equals bold italic n bold italic c subscript bold v bold increment bold italic T  --------------- eq (4)

where n is number of moles

The above equation comes from the relation, increment U equals q plus w (where U is internal energy and q is heat) for adiabatic process heat exchanged is zero, so work become equal to change in internal energy.

Given data,

V1= 1.6 L

V= 5.6 L

T1 = 333 K

T2 --- we have to find

cv = 28.05 J K-1mol-1

n = 1.63 moles

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