A diatomic gas is heated at constant at constant pressure. What fraction of the heat energy is used to increase the internal energy ?

1 kg of water is heated from 40 C to 70 C, If its volume remains constant, then the change in internal energy is (specific heat of water = 4148 J${kg}^{-1}{K}^{-1})$

The internal energy of compressed real gas, as  compared to that of the ideal gas at the same temperature is

The molar enthalpy change for $H_{2}O(1)\rightleftharpoons H2O(g)$ at $373$K and $1$ atm is $41$kJ/mol. Assuming ideal behavior, the internal energy change for vaporization of $1$ mol of water at $373$K and $1$ atm in kJ $mo{l}^{-1}$ is $?$

$100g$ of water is heated from ${30}^{o}C$ to ${50}^{o}C$. Ignoring the slight expansion of water, the change in its internal energy is (Specific heat of water is $4200J$ ${kg}^{-1}$ $K^{-1}$)

In a thermodynamic process, a system absorbs 2 k cal of heat and at the same time does 800 J of work. The change in internal energy of the system is

An ideal monoatomic gas undergoes a process in which its internal energy U and density $\rho$ vary as $U\rho =constant.$ The ratio of change in internal energy and the work done by the gas is

In a thermodynamic system working subtance is ideal gas, its internal energy is in the from of

Internal energy of an ideal gas depends on: