When $0.5 \ g$ of sulphur is burnt to $SO_2$,$4.6 \ kJ$ of heat is liberated. What is the enthalpy of formation of sulphur dioxide in $kJ \ mol^{-1}$?

What is the heat of atomisation of $P_4O_{6(s)}$?
Given that the heat of sublimation of $P_4O_6$ is $x \ kJ/mol$ and the $P-O$ bond energy is $y \ kJ/mol$.

Energy required to dissociate $16 \ g$ of oxygen gas $(O_2)$ into free atoms is $x \ kJ$. The heat of atomisation of oxygen is:

The enthalpy of neutralization is about $57.3 \ kJ$ for the pair:

The bond enthalpies of heavy hydrogen $(D-D)$, oxygen $(O=O)$, and heavy water $(D-O)$ are $+400$, $+498$, and $+490 \ kJ \ mol^{-1}$, respectively. The $\Delta_{r} H^{\circ}$ of the reaction to produce $D_2O$ is:

One mole of ethanol $(l)$ was completely burnt in oxygen to form $CO_{2(g)}$ and $H_2O_{(l)}$. What is the $\Delta_r H^{\ominus}$ (in $kJ \ mol^{-1}$) for this reaction?
(The standard enthalpy of formation $(\Delta_f H^{\ominus})$ of $C_2H_5OH_{(l)}$,$CO_{2(g)}$ and $H_2O_{(l)}$ is respectively $-277, -393$ and $-286 \ kJ \ mol^{-1}$.)