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1. For the equilibrium reaction \(P \rightleftarrows 2 Q\), at \(623^{\circ} \text{C}\), the following data was reported.
 

The equilibrium is established at time = 40 min when the temperature is 1519°C. Throughout the experiment, the partial pressure of P is maintained at 2 atm.
The ratio of the Gibbs free energy change at 623°C and 1519°C is:

1.	\(14\)	2.	\(\dfrac{1}{14}\)
3.	\(16\)	4.	\(\dfrac{1}{16}\)

2. Given the following transformation:
\({BaCO}_3(s) \longrightarrow {BaO}(s)+{CO}_2 (g)\)
Which of the following statements is/are correct for the above transformation?

I.	Phase transition
II.	Allotropic change
III.	\(\Delta H= +ve\)
IV.	\(\Delta S _{\text {sys }}= +ve\)

1. I, II and III
2. I, III and IV
3. I and III
4. III and IV

3. Given that the enthalpy of atomisation for \(Br_{2(l)}\) is \(x ~kJ/mol\) and the bond enthalpy for   \(Br_2 \) is \(y~kJ/mol,\) how are \(\text{x} ~\text{and}~ \text{y}\) related?
1.  \(x=y\)
2.  \(x<y\)
3. Not related
4.  \(x>y\)

4. A gas \(\text ({ Molar~ mass } =280~ g)\) was burnt in excess \(\mathrm{O_2}\) in a constant volume calorimeter, and during combustion, the temperature of the calorimeter increased from \(298.0 \mathrm{~K} \text { to } 298.45 \mathrm{~K} \text {. }\) If the heat capacity of the calorimeter is \(2.5 \mathrm{~kJ} \mathrm{~K}^{-1}\) and the enthalpy of combustion of the gas is \(9 \mathrm{~kJ} \mathrm{~mol}^{-1}\), then the amount of gas burned is:
1. \(35 \mathrm{~g}\)
2. \(24 \mathrm{~g}\)
3. \(67 \mathrm{~g}\)
4. \(81 \mathrm{~g}\)

5.