Calculate the work $\left(\mathrm{in} \mathrm{kJ}\right)$ of an isobaric reversible expansion of three moles of an ideal gas while it is heated from $298 \mathrm{K}$ to $400 \mathrm{K}$.

Calculate the work $\left(\mathrm{in} \mathrm{kJ}\right)$ of an isothermal reversible expansion of three moles of water vapour from $5.0\times {10}^4$ to $2.0\times {10}^4 \mathrm{Pa}$ at $330 \mathrm{K}$.

The heat of combustion of graphite at $298 \mathrm{K}$ is $-393.795 \mathrm{kJ}/\mathrm{mol}$, while that of diamond's combustion at the same temperature is $-395.692 \mathrm{kJ}/\mathrm{mol}$. The specific heats for these substances are $720.83$ and $505.58 \mathrm{J} {\mathrm{kg}}^{-1} {\mathrm{K}}^{-1}$, respectively. Calculate the heat of graphite's transformation into diamond in $\mathrm{kJ}/\mathrm{mol}$ at $298 \mathrm{K}$.

Diborane is formed from the elements as shown in equation $\left(1\right)$.

Given that,  $2\mathrm{B}\left(\mathrm{s}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\to {\mathrm{B}}_2{\mathrm{H}}_6\left(\mathrm{g}\right)$    ...$\left(1\right)$

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\to {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right) {\mathrm{\Delta H}}_1^0=44 \mathrm{kJ}$

$2\mathrm{B}+3/2{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{B}}_2{\mathrm{O}}_3\left(\mathrm{s}\right) {\mathrm{\Delta H}}_2^0=-1273 \mathrm{kJ}$

${\mathrm{B}}_2{\mathrm{H}}_6\left(\mathrm{g}\right)+3{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{B}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right) {\mathrm{\Delta H}}_3^0=-2035 \mathrm{kJ}$

${\mathrm{H}}_2\left(\mathrm{g}\right)+1/2{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right) {\mathrm{\Delta H}}_4^0=286 \mathrm{kJ}$

the ${\mathrm{\Delta H}}^0$ for the reaction $\left(1\right)$ is: