If $5 \ kJ$ of work is done on the system and $1 \ kJ$ of heat is released by the system,find the change in internal energy in $kJ$.

$A$ piston filled with $0.04 \ mol$ of an ideal gas expands reversibly from $50.0 \ mL$ to $375 \ mL$ at a constant temperature of $37.0 \ ^oC$. As it does so,it absorbs $208 \ J$ of heat. The values of $q$ and $w$ for the process will be
$(R = 8.314 \ J/mol \ K) \ (\ln 7.5 = 2.01)$

What is the final temperature of $0.10 \, mol$ monoatomic ideal gas that performs $75 \, cal$ of work adiabatically if the initial temperature is $227 \, ^oC$? .......$K$ (use $R = 2 \, cal \cdot K^{-1} \cdot mol^{-1}$)

$A$ system gives out $x \ J$ of heat and does $y \ J$ of work on its surroundings. What is the internal energy change?

When a system absorbs $8 \ kJ$ of heat and does $2.2 \ kJ$ of work on the surroundings,calculate the internal energy change. (in $kJ$)

Observe the following reaction: $ABO_{3(s)} \xrightarrow{1000 \ K} AO_{(s)} + BO_{2(g)}$. $\Delta_{r} H$ for this reaction is $x \ kJ \ mol^{-1}$. What is its $\Delta_{r} U$ (in $kJ \ mol^{-1}$) at the same temperature? $(R = 8.3 \ J \ mol^{-1} \ K^{-1})$