CORRECT representation of the heat supplied at a constant pressure and constant volume in gaseous reaction is:
(${\mathrm{n}}_1$=sum of the stoichiometric coefficient of reactants and ${\mathrm{n}}_2$= sum of the stoichiometric coefficient of products)

At constant $\mathrm{T}$ and $\mathrm{P},$ which one of the following statements is CORRECT for the reaction?

$\mathrm{CO}\left(\mathrm{g}\right)\mathrm{+}\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\stackrel{}{\to }{\mathrm{CO}}_2\left(\mathrm{g}\right)$

In a reaction,

${\mathrm{CO}}_{2\left(\mathrm{g}\right)}+{\mathrm{H}}_{2\left(\mathrm{g}\right)}\stackrel{}{\to }{\mathrm{CO}}_{\left(\mathrm{g}\right)}+{\mathrm{H}}_{\mathrm{2}}{\mathrm{O}}_{\left(\mathrm{g}\right)}\mathrm{;}$
$∆\mathrm{H} = +2.8 \mathrm{kJ}$ at constant pressure. The heat of reaction at constant volume is ______ .

For the reaction,

${\mathrm{CH}}_{\mathrm{3}}{\mathrm{COOH}}_{\left(\mathrm{l}\right)}+2{\mathrm{O}}_{2\left(\mathrm{g}\right)}\stackrel{}{\rightleftharpoons }2{\mathrm{CO}}_{2\left(\mathrm{g}\right)}+2{\mathrm{H}}_{\mathrm{2}}{\mathrm{O}}_{\left(\mathrm{l}\right)}$
at $25°\mathrm{C}$ and $1 \mathrm{atm}$ pressure, $∆\mathrm{H} = – 874 \mathrm{kJ},$ Then the change in internal energy $(∆\mathrm{U})$ is?

For the reaction,

${\mathrm{C}}_{\mathrm{3}}{\mathrm{H}}_{8 \left(\mathrm{g}\right)}+5{\mathrm{O}}_{2 \left(\mathrm{g}\right)}\mathrm{ }\stackrel{}{\to }3{\mathrm{CO}}_{2 \left(\mathrm{g}\right)} +3{\mathrm{H}}_{\mathrm{2}}{\mathrm{O}}_{ \left(\mathrm{l}\right)}$
at constant temperature, $∆\mathrm{H}-∆\mathrm{U}$ is      
 

The difference between the heat of reaction at constant pressure and constant volume for the reaction.
${\mathrm{C}}_{ \left(\mathrm{s}\right)}\mathrm{+}\frac{1}{2}{\mathrm{O}}_{2 \left(\mathrm{g}\right)}\stackrel{}{\to }{\mathrm{CO}}_{2 \left(\mathrm{g}\right)}$ is: $\mathrm{R}= 2 \mathrm{Cal}/\mathrm{mole}/\mathrm{K}$