Does the internal energy of an ideal gas change in an adiabatic process?

Specific heat of a gas undergoing adiabatic change is

$1 \, \text{kmol}$ of an ideal gas is compressed adiabatically,requiring $146 \, \text{kJ}$ of work. During this process,the temperature of the gas increases by $7^o \text{C}$. The gas is: $(R = 8.3 \, \text{J mol}^{-1} \text{K}^{-1})$

An ideal gas in a cylinder is compressed adiabatically to one-third of its original volume. $A$ work of $45 \,J$ is done on the gas by the process. The change in internal energy of the gas and the heat flowed into the gas, respectively are

$A$ cylinder with a movable piston contains $3$ moles of hydrogen at standard temperature and pressure. The walls of the cylinder are made of a heat insulator,and the piston is insulated by having a pile of sand on it. By what factor does the pressure of the gas increase if the gas is compressed to half its original volume?

During an adiabatic process, the pressure is proportional to the cube of the temperature. Then ${C_p}/{C_v}$ is . . . . . . .