Consider the reaction $2H_2S(g) + 3O_2(g) \rightarrow 2H_2O(l) + 2SO_2(g)$. The magnitude of enthalpy change for the reaction in $\text{kJ mol}^{-1}$ is . . . . . . . (Nearest integer). Given: $\Delta_f H^\circ(H_2S) = -20.1 \text{ kJ mol}^{-1}$,$\Delta_f H^\circ(H_2O) = -286.0 \text{ kJ mol}^{-1}$,$\Delta_f H^\circ(SO_2) = -297.0 \text{ kJ mol}^{-1}$

Given the bond energies of $N \equiv N$,$H - H$ and $N - H$ bonds are $945$,$436$ and $391 \ kJ \cdot mol^{-1}$ respectively,the enthalpy of the following reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$ is ...... $kJ$.

Enthalpy of formation of $CO_{(g)}$ and $CO_{2(g)}$ are $-110 \ kJ \ mol^{-1}$ and $-393 \ kJ \ mol^{-1}$ respectively. The enthalpy of combustion of $CO$ (in $kJ \ mol^{-1}$) is:

In an exothermic reaction,$\Delta H$ is

What will be the amount of heat evolved by burning $0.4 \ mol$ of methane? (Given heats of formation of $CH_4$,$CO_2$,and $H_2O$ are $-75$,$-400$,and $-240 \ kJ \ mol^{-1}$ respectively) ..... $kJ$

What will be the $C-H$ bond enthalpy if:
$CH_{4(g)} + 2O_{2(g)} \rightarrow CO_{2(g)} + 2H_2O_{(l)};$ $\Delta H = -890 \, kJ$
$CO_{2(g)} \rightarrow C_{(graphite)} + O_{2(g)};$ $\Delta H = 393 \, kJ$
$2H_2O_{(l)} \rightarrow 2H_{2(g)} + O_{2(g)};$ $\Delta H = 571 \, kJ$
$2H_{2(g)} \rightarrow 4H_{(g)};$ $\Delta H = 871 \, kJ$
$C_{(graphite)} \rightarrow C_{(g)};$ $\Delta H = 716 \, kJ$