The combustion of $1 \, \text{mol}$ of methanol in the presence of $O_2$ releases $723 \, \text{kJ mol}^{-1}$ of heat. If $1 \, \text{mol}$ of $O_2$ is used during this process,how much heat in $\text{kJ}$ will be produced?

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)

The amount of heat evolved when $500 \text{ cm}^{3}$ of $0.1 \text{ M } HCl$ is mixed with $200 \text{ cm}^{3}$ of $0.2 \text{ M } NaOH$ is (in $\text{ kJ}$)

What is the value of $PV$ type of work for the following reaction at $1 \ bar$ pressure (in $J$)? The reaction is: $C_2H_4(g) + HCl(g) \rightarrow C_2H_5Cl(g)$. Given volumes are $200 \ mL$ of $C_2H_4$ and $150 \ mL$ of $HCl$.

The amount of $BaSO_4$ formed upon mixing $100 \ mL$ of $20.8 \%$ $BaCl_2$ solution with $50 \ mL$ of $9.8 \%$ $H_2SO_4$ solution will be ............. $g$
( $Ba = 137, Cl = 35.5, S = 32, H = 1$ and $O = 16$ )

The heat of neutralisation of a strong acid and a strong base is $13.7 \ kcal$. The heat released when $0.6 \ mole$ $HCl$ solution is added to $0.25 \ mole$ of $NaOH$ is: (in $kcal$)