Heat and Internal Energy

Internal energy of an ideal gas depends on

One mole of argon is expanded according to process equation $P{V}^{1.5}=$ constant and its temperature falls by $26 \mathrm{K},$ then

A thermally insulated vessel containing diatomic gas of molar mass $M$ is moving with velocity $v.$ The temperature of gas is $T.$ If it is suddenly stopped, then

If molar heat capacity of a gas (monoatomic) in a certain process is $4 R$, if $\Delta Q$ amount of heat is given to this gas, then rise in internal energy of gas is given by

A mixture of gases contains $4$ moles of oxygen and $2$ moles of argon at absolute temperature $T.$ The total internal energy of this system (neglecting vibrations) is $[R=$ universal gas constant ]

Total kinetic energy of molecules of a gas sample varies as $\mathrm{K}.\mathrm{E}.=\frac{7}{4}nRT$. This sample contains

A sample contains $N$ moles of a diatomic gas at temperature $T.$ Molecules of gas get dissociated into atoms temperature remaining constant, find change in internal energy of gas.

Two moles of an ideal gas undergoes adiabatic process and changes its state from $(P_1, V_1, T_1)$ to $(P_2, V_2, T_2)$. The change in internal energy of the gas will be