When $500 \ J$ of heat is supplied to a system at constant volume,the temperature of the system increases from $20^oC$ to $25^oC$. The change in internal energy of the system is ...... $J$.

The relation $q = -w$ is $NOT$ true for which of the following processes?

In a $1 \, L$ container,$2 \, mol$ of $CO$ and $1 \, mol$ of $O_2$ are taken. They react according to the equation: $2CO(g) + O_2(g) \rightarrow 2CO_2(g)$,$\Delta H = -560 \, kJ$. Given that $1 \, atm \cdot L = 0.1 \, kJ$,and the pressure changes from $70 \, atm$ to $40 \, atm$ at $500 \, K$,calculate the value of $\Delta U$ in $kJ$.

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 $kJ$)?

Which of the following relations is correct for the internal energy change $(\Delta U)$ in a process occurring at constant volume?

Identify the state function among the following.