For the reaction $CH_3COOH_{(l)} + 2O_{2(g)} \rightleftharpoons 2CO_{2(g)} + 2H_2O_{(l)}$ at $25\,^{\circ}C$ and $1\,atm$ pressure,$\Delta H = -874\,kJ.$ Then the change in internal energy $(\Delta E)$ is $...\,kJ$

In a process,the work done by the system is equal to the change in its internal energy. Then the process will be ...........

What is the value of $\Delta H - \Delta U$ for the formation of $2$ moles of ammonia from $H_{2(g)}$ and $N_{2(g)}$?

$A$ sample of gas absorbs $4000 \ kJ$ of heat and the surrounding does $2000 \ J$ of work on the sample. What is the value of $\Delta U$ (in $kJ$)?

One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27\, ^{\circ}C$. If the work done during the process is $3\, kJ$,then the final temperature of the gas is $(C_v = 20\, J\, K^{-1}\, mol^{-1})$ .....$K$

$A$ gas absorbs $100 \ J$ of heat and is simultaneously compressed by a constant external pressure of $1.5 \ atm$ from a volume of $8.0 \ L$ to $2.0 \ L$. The change in internal energy for the gas in Joules is $(1 \ L \cdot atm = 101.32 \ J)$.