In a process the pressure of a gas is inversely proportional to the square of the volume. If temperature of the gas is increased, then work done on the gas-

1. is positive

2. is negative

3. is zero

4. maybe positive

The enthalpies of formation of CO₂(g) and CO(g) at 298 K are in the ratio 2.57 : 1. For the reaction,

$C{O}_2\left(g\right)+C\left(s\right)\to 2 CO\left(g\right), ∆H=172.5 kJ,$
$∆H_f of CO\left(g\right) is$

1. -150.6 kJ mol^-1

2. -302.63 kJ mol^-1

3. -130.2 kJ mol^-1

4. -141.8 kJ mol^-1

In an adiabatic expansion the product of pressure and volume-

1. decreases

2. increases

3. remains constant

4. first increase then decreases

The molar entropy of the vapourization of acetic acid is\(14.4~ \mathrm{cal}~ \mathrm{K}^{-1} \mathrm{~mol}^{-1}\) at its boiling point ${118}^{\circ }C$. The latent heat of vapourization of acetic acid is-

100 ml of 0.3 M HCl solution is mixed with 100 ml of 0.35 M NaOH solution. The amount of heat liberated is

1. 7.3 kJ

2. 5.71 kJ

3. 10.42 kJ

4. 1.713 kJ

The quantity ${\delta }_q$ i.e. heat absorbed an infinitesimal process is

1. Dependent on the path of transformation

2. Dependent on the thermodynamic state of the system

3. Independent of both

4. An exact differential

An ideal gas absorbs 2000 cal of heat from a heat reservoir and does mechanical work equivalent to
4200 J. The change in internal energy of the gas is:

1. 3000 cal

2. 2000 cal

3. 1500 cal

4. 1000 cal

For an ideal gas four processes are marked as 1, 2, 3 and 4 on P-V diagram as shown in figure. The amount of heat supplied to the gas in the process 1, 2, 3 and 4 are Q₁, Q₂, Q₃ and Q₄ repectively, then correct order of heat supplied to the gas is

[AB is process-1, AC is process-2, AD is adiabatic process-3 and AE is process-4]

1. $Q_1>Q_2>Q_3>Q_4$

2. $Q_1>Q_2>Q_4>Q_3$

3.  $Q_1>Q_4>Q_2>Q_4$

4. $Q_1<Q_2<Q_3<Q_4$

The latent heat of vapourisation of water at ${25}^{\circ }C$ is 10.5 kcal mol^-1 and the standard heat of formation of liquid water is -68.3 kcal. The enthalpy change of the reaction

$H_2\left(g\right)+\left(1/2\right)O_2\left(g\right)\to H_{2}O\left(g\right)$ is therefore,

1. -57.8 kcal

2. -78.8 kcal

3. 78.8 kcal

4. -47.3 kcal

Which of the following thermodynamic quantities is an outcome of the second law of thermodynamics?

1. Work

2. Enthalpy

3. Internal energy

4. Entropy