Irreversible Adiabatic Expansion And Compression

Q. 1 mol of ammonia gas at ${27}^{o}C$ is expanded in adiabatic reversible condition to make volume 8 times ($\gamma =\frac{4}{3}$). Final temperature and work done respectively are:

1. 150K, 400cal
2. 150K, 900cal
3. 250K, 1000cal
4. 200K, 800cal

Q. In an adiabatic process, no transfer of heat takes place between system and surroundings. Choose the correct option for free expansion of an ideal gas under adiabatic condition from the following.

1. $△q=0,△T\ne 0,w=0$
2. $△q\ne 0,△T=0,w=0$
3. $△q=0,△T=0,w=0$
4. $△q=0,△T<0,w\ne 0$

Q. Which one of the following is applicable for an adiabatic expansion of an ideal gas?

1. $\Delta E=0$
2. $\Delta W=0$
3. $\Delta W=\Delta E$
4. $\Delta W=-\Delta E$

Q. An ideal gas in thermally insulated vessel at internal pressure $=p_1$, volume $=V_1$ and absolute temperature $=T_1$ expands irreversibly against zero external pressure, as shown in the diagram.
The final internal pressure, volume and absolute temperature of the gas are $p_2,V_{2}and{T}_2$ respectively.
For this expansion

1. q = 0
2. $T_2=T_1$
3. $p_2{V}_2=p_1{V}_1$
4. $p_2{V}_2^{\gamma }=p_1{V}_1^{\gamma }$

Q. An ideal gas having initial pressure P, volume V and temperature T is allowed to expand reversibly and adiabatically until its volume becomes 5.66 V, while its temperature decreases to $\frac{T}{2}$. Work done by the gas during expansion is given by $W=-XPV$. Find the value of $X$. (given $(5.66{)}^{0.4}=2$) Report the answer upto two decimals

Q. 20 litres of a monoatomic ideal gas at $0^{o}C$ and 20 $atm$ pressure is suddenly exposed to 1 $atm$ pressure and the gas expands adiabatically against this constant pressure to maximum possible volume. The final temperature and volume of the gas respectively are

1. T = 169 K, V = 247.5 L
2. T = 165 K, V = 247.5 L
3. T = 169 K, V = 257.5 L
4. none of these

Q. For an adiabatic, irreversible, free expansion which of the following is/are true

1. $\Delta H=0$
2. $\Delta T=0$
3. $\Delta U=0$
4. $\Delta P_{\mathrm{int}}=0$