Question

Calculate the work done when $1$ mol of an ideal gas is compressed reversibly from $1$ bar to $4$ bar at a constant temperature of $300K$:

• A. $+3.45kJ$
• B. $-8.02kJ$
• C. $+18.02kJ$
• D. $-14.01kJ$

Answer 1

The correct option is A $+3.45kJ$

$n=1$ mole

$P_1=1$ bar

$P_2=4$ bar

$T=300$ K

It is a reversible & isothermal process.

$\therefore$ work done $=-nRTln\left(\frac{P_1}{P_2}\right)$

$=-1\times 8.314\times 300\times ln\left(\frac{1}{4}\right)$

$=3457.69J$

$=3.457KJ$

As the ideal gas is compressed, $W>0$

$\therefore$ work done $=+3.457KJ$