Calculate the maximum possible heat which can be released if a $4 \ L$ aqueous solution is to be formed by mixing appropriate volumes of $2 \ M$ $NaOH$ and $3 \ M$ $H_2SO_4$ solution. Given $\Delta H_{\text{neutralisation, SA/SB}} = -14 \ kcal/mol$.

If the heat of combustion of methane is $-100 \ kJ/mol$,then calculate the heat evolved when $32 \ g$ of methane reacts with $32 \ g$ of oxygen. (in $kJ$)

$A$ $10.0 \, L$ vessel contains $O_2$ at a partial pressure of $600 \, torr$ and $H_2$ at a partial pressure of $400 \, torr$. The gases react according to the following equation upon electric sparking: $H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(g)}$. If the reaction goes to completion,which of the following is correct?

In the given reaction,$X + Y + 3 Z \rightleftharpoons XYZ_3$. If one mole of each of $X$ and $Y$ with $0.05 \ mol$ of $Z$ reacts to form the compound $XYZ_3$,calculate the yield of $XYZ_3$ in grams. (Given: Atomic masses of $X, Y$ and $Z$ are $10, 20$ and $30 \ amu$,respectively). (Nearest integer)

For the given reaction:
$CaCO_{3} + 2HCl \to CaCl_{2} + H_{2}O + CO_{2}$
If $90 \ g$ of $CaCO_{3}$ is added to $300 \ mL$ of $HCl$ solution which contains $38.55\%$ $HCl$ by mass and has a density of $1.13 \ g \ mL^{-1}$, then which of the following options is correct?
[Given molar masses of $H$, $Cl$, $Ca$, and $O$ are $1$, $35.5$, $40$, and $16 \ g \ mol^{-1}$ respectively]

The mass of $Mg_3N_2$ produced if $48 \ g$ of $Mg$ metal is reacted with $34 \ g$ $NH_3$ gas is:
$3Mg + 2NH_3 \to Mg_3N_2 + 3H_2$