$A$ system does $200 \, J$ of work and at the same time absorbs $150 \, J$ of heat. The magnitude of the change in internal energy is $..... \, J.$ (Nearest integer)

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? $(R = 8.3 \ J \ mol^{-1} \ K^{-1})$

In the reaction $H_2O_{(l)} \rightarrow H_2O_{(s)}$ at $0^{\circ}C$ and $1 \ atm$, the internal energy change is $-41 \ kJ / mol$. What will be the value of molar enthalpy change?

The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of $10 \ L$ to $20 \ L$ at $25 \, ^oC$ is

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

For the formation of carbon monoxide $(CO)$ from its elements at $298 \, K$,the value of $(\Delta H - \Delta U)$ in $J \, mol^{-1}$ will be: $(R = 8.314 \, J K^{-1} mol^{-1})$