Questions in thermodynamics

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	An adiabatic process occurs at constant
	A polyatomic gas $\left( \gamma =\frac{4}{3} \right)$ is compressed to $\frac{1}{8}$ of its volume adiabatically. If its initial pressure is ${{P}_{o}}$, its new pressure will be
	For adiabatic processes $\left( \gamma =\frac{{{C}_{p}}}{{{C}_{v}}} \right)$
	An ideal gas is expanded adiabatically at an initial temperature of $300 K$ so that its volume is doubled. The final temperature of the hydrogen gas is $(\gamma =1.40)$
	A given system undergoes a change in which the work done by the system equals the decrease in its internal energy. The system must have undergone an
	During the adiabatic expansion of 2 moles of a gas, the internal energy was found to have decreased by 100 J. The work done by the gas in this process is
	In an adiabatic expansion of a gas initial and final temperatures are${{T}_{1}}$ and ${{T}_{2}}$ respectively, then the change in internal energy of the gas is
	Helium at ${{27}^{o}}C$ has a volume of 8 litres. It is suddenly compressed to a volume of 1 litre. The temperature of the gas will be $[\gamma =5/3]$
	A cycle tyre bursts suddenly. This represents an
	One mole of helium is adiabatically expanded from its initial state $({{P}_{i}},{{V}_{i}},{{T}_{i}})$ to its final state $({{P}_{f}},{{V}_{f}},{{T}_{f}})$. The decrease in the internal energy associated with this expansion is equal to