For an isochoric process,the first law of thermodynamics can be expressed as:

For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$ at $298 \ K$,the enthalpy change $(\Delta H)$ is $-92.38 \ kJ$. What will be the internal energy change $(\Delta U)$ at $298 \ K$ in $kJ$?

Identify from the following reactions the one that exhibits negative work done by the system.

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

In an adiabatic expansion of an ideal gas,which of the following relations holds true?

If $Q$ is the heat liberated from the system and $W$ is the work done on the system,then the first law of thermodynamics can be written as: