S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: Thermodynamics, Exercise 1: PROBLEMS FOR PRACTICE

$500 \mathrm{joules}$ of the heat was supplied to a system at constant volume. It resulted in the increase of the temperature of the system from $20°$$\mathrm{C}$ to $25°\mathrm{C}$. What is the change in internal energy of the system?

What would be the work done on/by the system if the internal energy of the system falls by $100 \mathrm{joules}$ even when $200 \mathrm{joules}$ of heat is supplied to it?

Calculate the work done when $1.0 \mathrm{mol}$ of water at $373 \mathrm{K}$ vaporizes against an atmospheric pressure of $1.0 \mathrm{atm}$. Assume the ideal gas behaviour.

Two moles of an ideal gas at $2 \mathrm{atm}$ and $27°\mathrm{C}$ are Compressed isothermally to half the volume by an external pressure of $4 \mathrm{atm}$. Calculate $\mathrm{W}, \mathrm{q}$ and $∆\mathrm{U}$.