One mole of a monoatomic ideal gas at an initial temperature of T K undergoes a reversible adiabatic expansion from an initial volume of 1 L to a final volume of 2 L. Find the final temperature of the gas.

1. T/(2)^2/3                                         

2. T + 2/(3x0.0821)

3. T                                                   

4. T - 3/(2x0.0821)

Find the correct relation between work done and change in internal energy during the adiabatic expansion of an ideal gas.

1. W = –ΔE

2. W = ΔE

3. ΔE = 0

4. W = 0

Equal volumes of monoatomic and diatomic gases at same initial temperature and pressure are mixed. The ratio of specific heats of the mixture (C_p/C_v) will be [AFMC 2002]

(1) 1

(2) 2

(3) 1.67

(4) 1.5

In an isobaric process, the ratio of heat supplied to the system (dQ) and work done by the system (dW) for diatomic gas is:

1. 1 : 1

2. 7 : 2

3. 7 : 5

4. 5 : 7

One mole of hydrogen gas at ${25}^{\circ }C$ and 1 atm pressure is heated at constant pressure until its volume has doubled. Given that $C_v$ for hydrogen is 3.0 cal deg^-1 mol^-1, the $∆H<mspace\; width="1em"></mspace>$and $∆E$ for this process are-

1. $∆H<mspace\; width="1em"></mspace>$= 1490 cal and $∆E$ = 894 cal

2. $∆H<mspace\; width="1em"></mspace>$= $∆E$= 1490 cal

3. $∆H<mspace\; width="1em"></mspace>$= 894 cal and $∆E$= 1490 cal

4. $∆H<mspace\; width="1em"></mspace>$= $∆E$= 894 cal