If $\Delta G$ and $\Delta S$ for the reaction $A_{(g)} \rightarrow B_{(g)} + 2C_{(g)}$ at $2000 \ K$ are $-40 \ kJ \ mol^{-1}$ and $0.22 \ kJ \ K^{-1} \ mol^{-1}$ respectively,the change in internal energy for the same reaction approximately (in $kJ \ mol^{-1}$) is

For a spontaneous process, the correct statement$(s)$ is (are):

Which of the following is incorrect?

Consider the following statements:
$(A)$ Entropy of a perfect crystalline solid at absolute zero approaches zero.
$(B)$ For spontaneity of a reaction at constant temperature and pressure, $T\Delta S > \Delta H$ (where $\Delta H$ is positive).
Identify the correct answer from the options given below.

For a dimerization reaction,$2 A_{(g)} \rightarrow A_{2(g)}$ at $298 \ K$,$\Delta U^{\ominus} = -20 \ kJ \ mol^{-1}$,$\Delta S^{\ominus} = -30 \ J \ K^{-1} \ mol^{-1}$,then the $\Delta G^{\ominus}$ will be........ $J$

Which of the following is not a correct statement?