Part $2$

Solid ammonium nitrite decomposes to form nitrogen gas and water vapour. The

decomposition releases $224kJ$ per mole of ammonium nitrite decomposed.

a$.$ Write the balanced equation for this reaction including the energy term in the

equation.

b$.$ Write the balanced equation for the reaction and use $H$ notation for the energy

term.

Consider the combustion of nitrogen monoxide:

$NO(g)+\frac{1}{2}{O}_2(g)longrightarrowN{O}_2(g),H=-56\mathrm{.}5k\frac{J}{m}ol$

How much heat would be released by the combustion of $65g$ of $NO(g)?$

Consider the double displacement reaction:

$Na2O(s)+2HI(g)longrightarrow2$NaI$(s)+H_{2}O(),H=-502\mathrm{.}1k\frac{J}{m}ol$

If $9\mathrm{.}00g$ of Nal$(s)$ are formed by this process, how much heat will be released?