Questions in thermodynamics

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	A gas for which $\gamma =1.5$is suddenly compressed to$\frac{1}{4}$th of the initial volume. Then the ratio of the final to the initial pressure is
	One mole of an ideal gas with $\gamma =1.4$, is adiabatically compressed so that its temperature rises from 27°C to 35°C. The change in the internal energy of the gas is $(R=8.3\,J/mol.K)$
	The volume of a gas is reduced adiabatically to $\frac{1}{4}$ of its volume at 27°C, if the value of $\gamma =1.4,$ then the new temperature will be
	During an adiabatic expansion of 2 moles of a gas, the change in internal energy was found –50J. The work done during the process is
	Adiabatic modulus of elasticity of a gas is $2.1\times {{10}^{5}}N/{{m}^{2}}.$ What will be its isothermal modulus of elasticity $\left( \frac{{{C}_{p}}}{{{C}_{v}}}=1.4 \right)$
	For an adiabatic expansion of a perfect gas, the value of $\frac{\Delta P}{P}$ is equal to
	A gas expands under constant pressure $P$ from volume ${{V}_{1}}$to${{V}_{2}}$. The work done by the gas is
	When heat in given to a gas in an isobaric process, then
	One mole of a perfect gas in a cylinder fitted with a piston has a pressure $P$, volume $V$ and temperature $T$. If the temperature is increased by $1 K$ keeping pressure constant, the increase in volume is
	A gas is compressed at a constant pressure of $50N/{{m}^{2}}$ from a volume of $10{{m}^{3}}$ to a volume of $4{{m}^{3}}$. Energy of $100 J$ then added to the gas by heating. Its internal energy is