If $92 \ g$ of $Na$ reacts with water in an open vessel at $300 \ K$, what is the value of work done (in $J$)? $[$Assume ideal nature of the gaseous product$]$

When $3 \ mol$ of $Ar_{(g)}$ is supplied with $229 \ J$ of heat at constant pressure,the temperature of the sample increases by $2.55 \ K$. Calculate the molar heat capacity of the gas at constant volume.

What is the value of $\Delta S_{\text{total}}$ for the following reaction at $300 \ K$:
$Fe_{2}O_{3(s)} + 3CO_{(g)} \longrightarrow 2Fe_{(s)} + 3CO_{2(g)}$
$\Delta H^{\circ} = -25 \ kJ, \Delta S^{\circ} = 15 \ J \ K^{-1}$ (in $J \ K^{-1}$)

$A$ gas (Molar mass $= 280 \ g \ mol^{-1}$) was burnt in excess $O_2$ in a constant volume calorimeter and during combustion the temperature of calorimeter increased from $298.0 \ K$ to $298.45 \ K$. If the heat capacity of calorimeter is $2.5 \ kJ \ K^{-1}$ and enthalpy of combustion of gas is $9 \ kJ \ mol^{-1}$,then the amount of gas burnt is $...... \ g$. (Nearest Integer)

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 $J \, K^{-1} \, mol^{-1}$?

An ideal gas undergoes isothermal compression from $5\, m^3$ to $1\, m^3$ against a constant external pressure of $4\, Nm^{-2}$. Heat released in this process is used to increase the temperature of $1\, mole$ of $Al$. If molar heat capacity of $Al$ is $24\, J\, mol^{-1}\, K^{-1}$,the temperature of $Al$ increases by: