Which of the following equations is correct for the heat of sublimation?

The enthalpies of combustion of diamond and graphite are $-395.4 \, kJ$ and $-393.5 \, kJ$ respectively. The enthalpy of transformation of diamond to graphite is ..... $kJ$.

What is the quantity of heat evolved when $6 \ g$ of carbon combines with sulphur to form $CS_2$ according to the reaction $C + 2S \rightarrow CS_2 \quad \Delta H = 92 \ kJ \ mol^{-1}$ (in $kJ$)?

Standard molar enthalpy of formation of $CO_2$ is equal to

The value of the enthalpy of neutralization of an acid and a base is significant only when $......$

The enthalpy of combustion of methane,graphite and dihydrogen at $298 \, K$ are $-890.3 \, kJ \, mol^{-1}$,$-393.5 \, kJ \, mol^{-1}$ and $-285.8 \, kJ \, mol^{-1}$ respectively. The enthalpy of formation of $CH_{4(g)}$ will be:
$(i) -74.8 \, kJ \, mol^{-1}$
$(ii) -52.27 \, kJ \, mol^{-1}$
$(iii) +74.8 \, kJ \, mol^{-1}$
$(iv) +52.26 \, kJ \, mol^{-1}$