If $65 \ kJ$ of work is done on the system and it releases $25 \ kJ$ of heat,what is the change in internal energy of the system (in $kJ$)?

If $\Delta H$ is the change in enthalpy and $\Delta E$ is the change in internal energy accompanying a gaseous reaction,which of the following is true?

For the gaseous reaction $A_{(g)} + 3B_{(g)} \rightarrow 3C_{(g)} + 3D_{(g)}$,the value of $\Delta U = 17 \, Kcal$ at $27 \, ^oC$. Assuming $R = 2 \, cal \, K^{-1} \, mol^{-1}$,the value of $\Delta H$ for the above reaction will be ....... $Kcal$.

If $1 \ L$ of an ideal gas at a pressure of $20 \ atm$ expands isothermally and reversibly to a final volume of '$X$' $L$ by absorbing $92.12 \ L \ atm$ heat,'$X$' (in $L$) is

Calculate the change in internal energy of the system if $20 \ kJ$ of work is done on the system and it releases $10 \ kJ$ of heat in a particular reaction. (in $kJ$)

Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas? (Assume non-expansion work is zero)