During compression of a spring,the work done is $10 \ kJ$ and $2 \ kJ$ escaped to the surroundings as heat. The change in internal energy,$\Delta U$ (in $kJ$),is

One mole of gas absorbs $200 \ J$ of heat at constant volume,then its temperature rises from $298 \ K$ to $308 \ K$. The change in internal energy will be $... \ J$.

$A$ piston filled with $0.04\, mol$ of an ideal gas expands reversibly from $50.0\, mL$ to $375\, mL$ at a constant temperature of $37\, ^oC$. It absorbs $208\, J$ of heat in this process. The value of $q$ and $w$ for the process will be: $(R = 8.314\, J / mol\, K)$ $(\ln 7.5 = 2.01)$

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 $...... \ cal$.

At $1 \ bar$ pressure,a gas has a volume of $0.6 \ L$. If this gas gains $122 \ J$ of heat at $1 \ bar$ pressure,its volume becomes $2 \ L$. Calculate its internal energy change. [Given: $1 \ L \cdot bar = 101.32 \ J$]

What is the change in internal energy if a system does $140 \ kJ$ of work on the surroundings and $40 \ kJ$ of heat is added to the system (in $kJ$)?