Enthalpy change for freezing of $1 \ g$ of water at $1 \ bar$ and $0^{\circ} C$ is $334 \ J$. Calculate the internal energy change in $J$ when $1 \ g$ of water is converted into ice?

For the reaction $H_{2}F_{2(g)} \rightarrow H_{2(g)} + F_{2(g)}$,$\Delta U = -59.6 \ kJ \ mol^{-1}$ at $27^{\circ} C$. The enthalpy change for the above reaction is $(-)$ $kJ \ mol^{-1}$ [nearest integer]. Given: $R = 8.314 \ J \ K^{-1} \ mol^{-1}$.

$A$ thermodynamic process $(B \rightarrow E)$ is shown in the graph below. The work done in this process is equal to the area under the curve. Identify the correct area representing the work done.

Which statement is correct?

Which among the following are intensive and extensive properties respectively?

When $2 \ mol$ of an ideal gas undergoes spontaneous expansion in a vacuum,the work done is ...... Joules.