The mathematical equation of the first law of thermodynamics for an isochoric process is:

The enthalpy of vapour is $10 \ kcal/mole$ higher than liquid at $350 \ K$ and $2 \ atm$. Under given conditions,the difference in internal energy of vapour and liquid will be $...... \ cal$.

For the reaction $C_{(s)} + O_{2_{(g)}} \rightarrow CO_{2_{(g)}}$,which of the following is true?

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 $kJ$)?

$A$ sample of gas expands against a constant external pressure of $1 \ atm$ from a volume of $2 \ L$ to $12 \ L$. During this process,it absorbs $600 \ J$ of heat. Calculate $\Delta E$ of the system.

If $100 \ L$ of gas is enclosed in a cylinder, absorbs $302.6 \ J$ of heat and expands to $200 \ L$ against a constant external pressure of $2 \ Pa$, calculate the internal energy change of the gas. (in $J$)