In a process, the pressure of an ideal gas is proportional to square of the volume of the gas. If the temperature of the gas increases in this process, then work done by this gas

In a process the pressure of a gas is inversely proportional to the square of the volume. If temperature of the gas increases, then work done by the gas:

In a process the pressure of a gas is inversely proportional to the square of the volume. If temperature of the gas increases, then work done by the gas:

In a process the pressure of a gas is inversely proportional to the square of the volume. If temperature of the gas increases, then work done by the gas:

During an adiabatic process, the pressure of a gas is found to be proportional to the square of its absolute temperature. The γ for the gas is

During an adiabatic process, the pressure of a gas is found to be proportional to the square of its absolute temperature. The γ for the gas is

If the pressure and the temperature of a gas change at constant volume, what is the work done by the gas?

In a thermodynamic process two moles of a monatomic ideal gas obeys PV^(–2)=constant . If temperature of the gas increases from 300 K to 400 K, then find work done by the gas (Where R = universal gas constant)

In a thermodynamic process two moles of a monatomic ideal gas obeys PV^(–2)=constant . If temperature of the gas increases from 300 K to 400 K, then find work done by the gas (Where R = universal gas constant)

When 1 mol of an ideal gas is compressed in a reversible isothermal process at T K, the pressure of the gas changes from 1 atm to 10 atm. In the process, if the work done by the gas be 5.744kJ, then T is-

For 1 mole of an ideal gas, during an adiabatic process, the square of the pressure of a gas is found to be proportional to the cube of its absolute temperature. The specific heat of the gas at constant volume is (R - universal gas constant)