If for a certain reaction ${∆}_{r}H$ is 30 kJ mol^–1 at 450 K, the value of ${∆}_{r}S$ (in JK^–1 mol^–1) for which the same reaction will be spontaneous at the same temperature is:

1. 70

2. –33

3. 33

4. -70

Consider the following processes :

                                       ∆H (kJ/mol)
½ A → B                            + 150
3B → 2C + D                      –125
E + A → 2D                        +350

For B + D → E + 2C, ∆H will be-

1. 325 kJ/mol 

2. 525 kJ/mol

3. –175 kJ.mol 

4. –325 kJ/mol

For vaporization of water at 1 atmospheric pressure, the values of ∆H and ∆S are 40.63 kJ mol^–1 and 108.8 JK^–1 mol^–1, respectively. The temperature when Gibbs energy change (∆G) for this transformation will be zero, is -

1. 393.4 K

2. 373.4 K

3. 293.4 K

4. 273.4 K

Three moles of an ideal gas expanded spontaneously into vaccum. The work done will be

1. 3 Joules

2. 9 Joules

3. Zero

4. Infinite

The following two reactions are known$$\begin{gathered} F{e}_2{O}_3\left(s\right)+3CO\left(g\right)\to 2Fe\left(s\right)+3C{O}_2\left(g\right); \\ ∆H=-26.88 kJ \\ FeO\left(s\right)+CO\left(g\right)\to Fe\left(s\right)+C{O}_2\left(g\right); \\ ∆H=-16.5 kJ \end{gathered}$$

The value of $∆$H for the following reaction

$F{e}_2{O}_3\left(s\right)+CO\left(g\right)\to 2FeO\left(s\right)+C{O}_2\left(g\right)$ is

1. -43.3 kJ

2. -10.3 kJ

3. +6.2 kJ

4. +10.3 kJ

Match List – I (Equations) with List – II (Type of processes) and select the correct option.

    List –I                                    List – II
    Equation                             Type of processes

(a) K_p > Q                           (i) Non spontaneous
(b) ∆G^º < RT ln Q                 (ii) Equilibrium
(c) K_p = Q                           (iii) Spontaneous and endothermic
(d) T > $\frac{∆H}{∆S}$                       (iv) Spontaneous

Options :
      (a)  (b)  (c)   (d)
1. (iii)  (iv)  (ii)   (i)
2. (iv)   (i)   (ii)   (iii)
3. (ii)    (i)   (iv)  (iii)
4. (i)    (ii)   (iii)  (iv)

Equal volumes of two monoatomic gases, A and B, at same temperature and pressure are mixed. The ratio of specific heats (Cp/Cv) of the mixture will be -
1.  1.50
2.  3.3
3.  1.67
4.  0.83

Entropy change in surroundings when 1.00 mol of $H_2{O}_{\left(l\right)}$ is formed under standard conditions. ${∆}_f{H}^{\theta }=-286 kJ mo{l}^{-1}$ is

$$\begin{gathered} 1. -959.73 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1} \\ 2. 234.98 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1} \\ 3. 959.73 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1} \\ 4. 312.56 \mathrm{J} {\mathrm{K}}^{-1 }{\mathrm{mol}}^{-1} \end{gathered}$$

The equilibrium constant for a reaction is 10. The value of $∆\mathrm{G}°$ will be-

($\mathrm{R} = 8.314 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1} ; \mathrm{T} = 300 \mathrm{K}$)

$$\begin{gathered} 1. -5.74 \mathrm{kJ} {\mathrm{mol}}^{-1} \\ 2. - 5.74 \mathrm{J} {\mathrm{mol}}^{-1} \\ 3. + 4.57 \mathrm{kJ} {\mathrm{mol}}^{-1} \\ 4. -57.4 \mathrm{kJ} {\mathrm{mol}}^{-1} \end{gathered}$$

For the reaction $2\mathrm{A} \left(\mathrm{g}\right) + \mathrm{B}\left(\mathrm{g}\right) \to 2\mathrm{D} \left(\mathrm{g}\right)$; $∆\mathrm{U}° = -10.5 \mathrm{kJ} \mathrm{and} ∆\mathrm{S}° = -44.1 \mathrm{J} {\mathrm{K}}^{-1}$ , the value of $∆\mathrm{G}°$ for the given reaction would be-

1. 1.6 J

2. - 0.16 KJ

3. 0.16 KJ

4. 1.6 KJ