At $25^{\circ} \text{C}$,$1 \text{ mole}$ of butane is combusted to form $CO_2$ and liquid $H_2O$. The work done is $...... \text{ L atm}$.

$500 \ J$ of energy is transferred as heat to $0.5 \ mol$ of Argon gas at $298 \ K$ and $1.00 \ atm$. The final temperature and the change in internal energy respectively are $:$ Given $: R = 8.3 \ J \ K^{-1} \ mol^{-1}$

For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$ at $977 \ ^oC$,given $\Delta H = 176 \ kJ \ mol^{-1}$,the value of $\Delta E$ is ............. $kJ$.

The value of $\Delta H_{transition}$ for $C(\text{graphite}) \rightarrow C(\text{diamond})$ is $1.9 \ kJ/mol$ at $25^{\circ}C$. The entropy of graphite is higher than the entropy of diamond. This implies that which of the following is incorrect $:-$

How many quantities have a similar unit as molar entropy?
$(i)$ Heat capacity
$(ii)$ Molar heat capacity
$(iii)$ Universal gas constant
$(iv)$ Specific heat capacity

The heat of combustion of naphthalene $(C_{10}H_8(s))$ at constant volume is $-5133 \, kJ \, mol^{-1}$. The value of enthalpy change is .... $J$ $(R = 8.314 \, J \, K^{-1} \, mol^{-1}, T = 298 \, K)$.