Two identical containers, A and B, contain the same ideal gas at the same pressure and volume. Container A undergoes an isothermal expansion, while container B undergoes an adiabatic expansion, both to the same final volume. Which container experiences a greater change in internal energy?

A system undergoes an adiabatic process where it does $100\,J$ of work on its surroundings. What is the change in its internal energy?

During the vaporization of 0.1 g of water at $100^\circ C$ and $1.013 imes 10^5 N m^{-2}$, the volume increases by 167.1 cc. If 54 cal of heat is absorbed during this process, how much work is done by the system?

Find the change in the entropy in the following process $100g$ of ice at ${0^ \circ }C$ melts when dropped in a bucket of water at ${50^ \circ }C$ (Assume temperature of water does not change)

Which of the following can not determine the state of a thermodynamic system

0.2 g of water at $100^\circ C$ and normal pressure ($1.013 imes 10^5 N m^{-2}$) requires 108 cal of heat energy to convert to steam at $100^\circ C$. If the volume of the steam produced is 334.2 cc, what is the change in internal energy of the sample?

A system goes from $A$ and $B$ via two processes $I$ and $II$ as shown in figure. If $\Delta {U_1}$ and $\Delta {U_2}$ are the changes in internal energies in the process $I$ and $II$ respectively, then

Air in a cylinder is suddenly compressed by a piston, which is then maintained at the same position. With the passage of

The $SI$ unit of mechanical equivalent of heat is

Compressed air in the tube of a wheel of a cycle at normal temperature suddenly starts coming out from a puncture. The air inside

In an isochoric process, the internal energy of a system increases by 50 J. What is the heat absorbed by the system?