Among the following the number of state variable is

Internal energy $\left(\mathrm{U}\right)$

Volume $\left(\mathrm{V}\right)$

Heat $\left(\mathrm{q}\right)$

Enthalpy $\left(\mathrm{H}\right)$

$\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right)+400 \mathrm{kJ}$

$\mathrm{C}\left(\mathrm{s}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to \mathrm{CO}\left(\mathrm{g}\right)+100 \mathrm{kJ}$

When coal of purity $60\%$ is allowed to burn in presence of insufficient oxygen, $60\%$ of carbon is converted into ' $\mathrm{CO}$' and the remaining is converted into '${\mathrm{CO}}_2$'.

The heat generated when $0.6 \mathrm{kg}$ of coal is burnt is

For independent process at $300 \mathrm{K}$.

The number of non-spontaneous process from the following is _____ .

One mole of an ideal monoatomic gas is subjected to changes as shown in the graph. The magnitude of the work done (by the system or on the system) is _______ J (nearest integer)

Given : log 2 = 0.3, ln 10 = 2.3

An athlete is given $100 \mathrm{g}$ of glucose $\left({\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\right)$ for energy. This is equivalent to $1800 \mathrm{kJ}$ of energy. The $50\%$ of this energy gained is utilized by the athlete for sports activities at the event. In order to avoid storage of energy, the weight of extra water he would need to perspire is $\mathrm{\_\_\_\_\_g}$ (Nearest integer) Assume that there is no other way of consuming stored energy.

Given : The enthalpy of evaporation of water is $45 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Molar mass of $\mathrm{C},\mathrm{H}\&\mathrm{O}$ are $12.1$ and $16 \mathrm{g} {\mathrm{mol}}^{-1}$.

$28.0$ L of ${\mathrm{CO}}_2$ is produced on complete combustion of $16.8 \mathrm{L}$ gaseous mixture of ethene and methane at $25°\mathrm{C}$ and $1$ atm. Heat evolved during the combustion process is $\mathrm{kJ}$

Given$:{\mathrm{\Delta H}}_{\mathrm{C}}\left({\mathrm{CH}}_4\right)=-900 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{\Delta H}}_{\mathrm{C}}\left({\mathrm{C}}_2{\mathrm{H}}_4\right)=-1400 \mathrm{kJ} {\mathrm{mol}}^{-1}$.