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Given
(\text{N}_{2}(\text{g}) + 3\text{H}_{2}(\text{g}) \rightarrow 2\text{NH}_{3}(\text{g}); \Delta_{r}H^{\circ} = –92.4 \text{ kJ mol}^{-1})
What is the standard enthalpy of formation of (\text{NH}_{3}) gas?

Calculate the standard enthalpy of formation of (\text{CH}_{3}\text{OH(l)}) from the following data:
(\text{CH}_{3}\text{OH (l)} + \frac{3}{2} \text{O}_{2}(\text{g}) \rightarrow \text{CO}_{2}(\text{g}) + 2\text{H}_{2}\text{O(l)} ; \Delta_{r}H^{\circ} = –726 \text{ kJ mol}^{-1})
(\text{C(graphite)} + \text{O}_{2}(\text{g}) \rightarrow \text{CO}_{2}(\text{g}) ; \Delta_{c}H^{\circ} = –393 \text{ kJ mol}^{-1})
(\text{H}_{2}(\text{g}) + \frac{1}{2} \text{O}_{2}(\text{g}) \rightarrow \text{H}_{2}\text{O(l)}; \Delta_{f} H^{\circ} = –286 \text{ kJ mol}^{-1}).

Calculate the enthalpy change for the process
(\text{CCl}_{4}(\text{g}) \rightarrow \text{C(g)} + 4 \text{Cl(g)})
and calculate bond enthalpy of (C – Cl) in (\text{CCl}_{4}(\text{g})).
(\Delta_{\text{vap}}H^{\circ}(\text{CCl}_{4}) = 30.5 \text{ kJ mol}^{-1}).
(\Delta_{f}H^{\circ} (\text{CCl}_{4}) = –135.5 \text{ kJ mol}^{-1}).
(\Delta_{a}H^{\circ} (\text{C}) = 715.0 \text{ kJ mol}^{-1}), where (\Delta_{a}H^{\circ}) is enthalpy of atomisation
(\Delta_{a}H^{\circ} (\text{Cl}_{2}) = 242 \text{ kJ mol}^{-1})

For an isolated system, (\Delta U = 0), what will be (\Delta S)?

For the reaction at (298) K,
(2A + B \rightarrow C)
(\Delta H = 400 \text{ kJ mol}^{-1}) and (\Delta S = 0.2 \text{ kJ K}^{-1} \text{mol}^{-1})
At what temperature will the reaction become spontaneous considering (\Delta H) and (\Delta S) to be constant over the temperature range.

For the reaction,
(2 \text{Cl(g)} \rightarrow \text{Cl}_{2}(\text{g})), what are the signs of (\Delta H) and (\Delta S)?

For the reaction
(2 \text{A(g)} + \text{B(g)} \rightarrow 2\text{D(g)})
(\Delta U^{\circ} = –10.5) kJ and (\Delta S^{\circ} = –44.1 \text{JK}^{-1}).
Calculate (\Delta G^{\circ}) for the reaction, and predict whether the reaction may occur spontaneously.

The equilibrium constant for a reaction is (10). What will be the value of (\Delta G^{\circ})? (R = 8.314 \text{ JK}^{-1} \text{mol}^{-1}), (T = 300) K.

Comment on the thermodynamic stability of (\text{NO(g)}), given
(\frac{1}{2} \text{N}_{2}(\text{g}) + \frac{1}{2}\text{O}_{2}(\text{g}) \rightarrow \text{NO(g)}; \Delta_{r}H^{\circ} = 90 \text{ kJ mol}^{-1})
(\text{NO(g)} + \frac{1}{2}\text{O}_{2}(\text{g}) \rightarrow \text{NO}_{2}(\text{g}): \Delta_{r}H^{\circ}= –74 \text{ kJ mol}^{-1})

10.

Calculate the entropy change in surroundings when (1.00) mol of (\text{H}_{2}\text{O(l)}) is formed under standard conditions. (\Delta_{f} H^{\circ} = –286 \text{ kJ mol}^{-1}).

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