G L Mittal and TARUN MITTAL Solutions for Chapter: Isothermal and Adiabatic Processes, Exercise 2: NUMERICALS

A certain mass of air $(\gamma = 1.5)$ at $27°C$ is compressed slowly to one fourth of its original volume. Find the final temperature.

A certain mass of air $(\gamma = 1.5)$  at $27°C$ is compressed suddenly to one-fourth of original volume find the final temperature of the compressed air.

A gas initially at atmospheric pressure and $15°\mathrm{C}$ compressed adiabatically until its volume remain one fourth of its original volume find out final pressure and temperature of gas. $(\gamma = 1.5)$

A monatomic ideal gas at $17 °\mathrm{C}$ is suddenly compressed to $\frac{1}{8}$ of its initial volume find the final temperature of the gas. Given for monatomic gas $\gamma = 5/3$.

 A gas, whose initial temperature is $27°C$, is compressed adiabatically to 8 times its initial pressure. If $\mathrm{\gamma } = 1.5$, find the rise in temperature in this transformation.

Two moles of oxygen at $0°C$ are compressed until the volume remains one-fourth of the initial value at the same temperature. Calculate the work done. $R = 8.31 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$.

An ideal gas of volume $1$ litre and at pressure $8$ atmospheres expands adiabatically until the pressure drops to 1 atmosphere. Find the final volume and work done. Given: $\gamma = 1.5,1$ atmosphere $= 1.013 x {10}^5 \mathrm{N} {\mathrm{m}}^{-2}$  and $1$ litre $= {10}^{-3} {\mathrm{m}}^3.$

One mole of oxygen at NTP has compressed adiabatically to $5$ atmospheres. What are the new temperature and the work done? Given : $\gamma = 1.4$ and $R = 8.31 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$.