For the reaction $N_{2(g)}N\_\{2(g)\}$ + $3H_{2(g)}3H\_\{2(g)\}$ = $2N{H}_{3(g)}2NH\_\{3(g)\}$ ; Which of the following is valid ?

The heat of combustion of carbon is 394 kJ $mo{l}^{-1}mol^\{-1\}$ . The heat evolved in combustion of $6.023\times 10^{22}6.023\; \backslash times\; 10\; ^\{22\}$ atoms of carbon is

Which of the reactions defines the heat of formation ?

$\mathrm{\Delta }{U}^{\circ }\backslash Delta\; U^\backslash circ$ of combustion of methane is -X kJ $mo{l}^{-1}mol^\{-1\}$ . The value of $\mathrm{\Delta }{H}^{\circ }\backslash Delta\; H^\backslash circ$ is

The enthalpy of combustion of 5(rhomic)is -297.4 kJ ${\text{mol}}^{-1}\mathrm{.}\backslash text\; \{mol\}^\{-1\}.$ The amount of sulphur required to produce 29.74 kJ of heat is

The heat of formation of $S{O}_{2(g)}SO\_\{2(g)\}$ and $S{O}_{3(g)}SO\_\{3(g)\}$ are -269 kJ $mo{l}^{-1}mol^\{-1\}$ and -395 kJ $mo{l}^{-1}mol^\{-1\}$ respectively the value of ΔH for the reaction $S{O}_{2(g)}+\frac{1}{2}{O}_{2(g)}\to S{O}_{3(g)}SO\_\{2(g)\}\; +\; \backslash frac\{1\}\{2\}O\_\{2(g)\}\; \backslash rightarrow\; SO\_\{3(g)\}$ is

The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are, -890.3 kJ $mo{l}^{-1}mol^\{-1\}$ , -393.5 kJ $mo{l}^{-1}mol^\{-1\}$ and -285.8 kJ $mo{l}^{-1}mol^\{-1\}$ respectively. Enthalpy of formation of $C{H}_{4(g)}CH\_\{4(g)\}$ will be

The enthalpies of formation of $N_2{O}_{(g)}N\_2\; O\_\{(g)\}$ and $N{O}_{(g)}NO\_\{(g)\}$ are 82 kJ $mo{l}^{-1}mol^\{-1\}$ and 90 kJ $mo{l}^{-1}mol^\{-1\}$ respectively. Then enthalpy of a reaction $2N_2{O}_{(g)}+O_{(g)}\to 4N{O}_{(g)}2N\_2\; O\_\{(g)\}\; +\; O\_\{(g)\}\; \backslash rightarrow\; 4NO\_\{(g)\}$ is ………

The heat of combustion of naphthalene $(C_{10}{H}_8)(C\_\{10\}\; H\_8\; )$ to $C{O}_{2}CO\_2$ gas and water vapour at 298 K and at constant pressure is $-5.1567\times 10^{6}J\mathrm{.}-5.1567\backslash times\; 10\; ^6\; J.$ The heat of combustion at constant volume at 298 K is $(R=8.314J{K}^{-1}mo{l}^{-1})(R\; =\; 8.314\; \backslash ,\; JK\; ^\{-1\}\backslash ,mol\; ^\{-1\})$ :

Given the reaction,

$2N{H}_3(g)\to N_{2(g)}+3H_{2(g)}\mathrm{△}H=92.6kJ2\; NH\; \_\; 3\; (g)\; \backslash rightarrow\; N\_\{2\; (g)\}\; +\; 3\; H\; \_\{2\; (g)\}\; \backslash triangle\; H\; =\; 92.6\; kJ$

The enthalpy of formation of $N{H}_{3}NH\_3$ is :