For the reaction,$N_{2(g)} + 3 H_{2(g)} \rightarrow 2 NH_{3(g)}$,$\Delta H$ is equal to

Calculate the change in enthalpy in a chemical reaction when work done is $-800 \ J$ and increase in internal energy is $600 \ J$. (in $J$)

According to the first law of thermodynamics,which of the following is correct? (Where $q =$ heat supplied to the system and $W =$ work done by the system)

$A$ 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
$(R = 8.314 \ J/mol \ K) \ (\ln 7.5 = 2.01)$

An ideal gas expands against a constant external pressure of $2 \ bar$ from $5 \ L$ to $8 \ L$ and absorbs $10 \ kJ$ of heat. What is $\Delta U$ of the system (in $J$)?

At a certain temperature, T(K), during a process, 500 J is absorbed by the system and work of 200 J is done by the system. Then change in internal energy of the system is: