What is the value of the increase in internal energy when a system does $8 \ J$ of work on the surroundings by supplying $40 \ J$ of heat to it (in $J$)?

Calculate the difference between $\Delta H$ and $\Delta U$ for the combustion of $n$-octane at $25^{\circ}C$. (in $kJ$)

Standard enthalpy of vaporisation $\Delta_{vap}H^o$ for water at $100\ ^oC$ is $40.66\ kJ\ mol^{-1}.$ The internal energy of vaporisation of water at $100\ ^oC$ (in $kJ\ mol^{-1}$) is ............... $kJ\ mol^{-1}$ (Assume water vapour to behave like an ideal gas)

What is the internal energy change when $62 \ J$ of work is done on the system and $128 \ J$ of heat is transferred to the surrounding (in $J$)?

When $1 \, \text{mol}$ of a gas is heated at constant volume,the temperature increases from $298 \, K$ to $308 \, K$. If the heat supplied to the gas is $500 \, J$,which of the following statements is correct?

For the reaction $CO_{(g)} + \frac{1}{2} O_{2(g)} \rightarrow CO_{2(g)}$ at constant temperature and pressure,which of the following statements is correct?