A molecule whose molar specific heat at high temperature, assuming ideal behaviour, is $9\mathrm{R}$ is:

Human being required $2500 \mathrm{Kcal}$ of energy per day

${\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}+12{\mathrm{O}}_2\to 12{\mathrm{CO}}_2+11{\mathrm{H}}_2\mathrm{O}; \mathrm{\Delta H}=-5.6\times {10}^6 \mathrm{J}/\mathrm{mol}$

Answer the following:

(i) Human being required ...... $\mathrm{kJ}$ of energy per day.
(ii) Amount of sucrose required per day and volume of ${\mathrm{CO}}_2$ evolved during the process [at $\mathrm{STP}$].

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:

An isolated box, equally partitioned contains two ideal gases $\mathrm{A}$ and $\mathrm{B}$ as shown:

When the partition is removed, the gases mix. The changes in enthalpy $\left(\mathrm{\Delta H}\right)$ and entropy $\left(\mathrm{\Delta S}\right)$ in the process, respectively, are: