For the reaction $2 Cl ( g ) \rightarrow Cl _{2}( g )$,the correct option is

The heats of combustion of $C_{(s)}$,$H_{2(g)}$,and $C_{2}H_{6(g)}$ are $-x_{1}$,$-x_{2}$,and $-x_{3}$ respectively. The heat of formation of $C_{2}H_{6(g)}$ is:

At constant volume,$5 \, mol$ of a gas shows an increase in temperature by $3.5 \, K$ upon providing $437.5 \, J$ of heat. What will be the molar heat capacity for the gas at constant pressure in $J \, K^{-1} \, mol^{-1}$?

Consider the following statements:
Statement-$I$: Both internal energy $(U)$ and work $(w)$ are state functions.
Statement-$II$: During the free expansion of an ideal gas into vacuum,the work done is zero.
The correct answer is:

One mole of an ideal gas at $900 \ K$ undergoes two reversible processes,$I$ followed by $II$,as shown in the graph. If the work done by the gas in the two processes is the same,the value of $\ln \frac{V_3}{V_2}$ is. . . . . . . . ($U$: internal energy,$S$: entropy,$p$: pressure,$V$: volume,$R$: gas constant). (Given: molar heat capacity at constant volume,$C_{V, m}$ of the gas is $\frac{5}{2} R$)

Which of the following is true for the reaction $H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$ at $100 ^oC$ and $1 \text{atm}$ pressure?