For irreversible expansion of an ideal gas under isothermal condition,the correct option is :

The ${\Delta _c}{U^\circ}$ of combustion of $CH_{4(g)}$ at a certain temperature is $-100 \ kJ/mol$. The value of ${\Delta _c}{H^\circ}$ is

For the process $H_2O_{(l)} (1 \, bar, 373 \, K) \rightarrow H_2O_{(g)} (1 \, bar, 373 \, K)$,identify the correct thermodynamic parameters.

$5$ moles of an ideal gas is expanded from $(10 \ L, 300 \ K)$ to $(20 \ L, 300 \ K)$ against a constant external pressure of $1.0 \ bar$. The only incorrect value of physical quantities for this change in state of the system,is-

For the complete combustion of methanol
$CH_3OH_{(l)} + \frac{3}{2} O_{2(g)} \rightarrow CO_{2(g)} + 2H_2O_{(l)}$
the amount of heat produced as measured by a bomb calorimeter is $726 \ kJ \ mol^{-1}$ at $27^{\circ}C$. The enthalpy of combustion for the reaction is $-x \ kJ \ mol^{-1}$,where $x$ is $.....$ (Nearest integer).
(Given: $R = 8.3 \ J \ K^{-1} \ mol^{-1}$)

Assuming the water vapour to be a perfect gas,calculate the internal energy change when $1 \ mol$ of water at $100^{\circ} C$ and $1 \ bar$ pressure is converted to ice at $0^{\circ} C$. Given the enthalpy of fusion of ice is $6.00 \ kJ \ mol^{-1}$ and heat capacity of water is $4.2 \ J \ g^{-1} {\circ} C^{-1}$.