Calculate the value of $\Delta G$ for the following reaction at $300 \ K$.
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$
$(\Delta H = 7 \ kJ, \Delta S = 24.8 \ J \ K^{-1})$

Which of the following conditions will always lead to a non-spontaneous change?

For the reaction at $298 \, K$,$2 A + B \rightarrow C$. Given $\Delta H = 400 \, kJ \, mol^{-1}$ and $\Delta S = 0.2 \, kJ \, K^{-1} \, mol^{-1}$. At what temperature will the reaction become spontaneous,considering $\Delta H$ and $\Delta S$ to be constant over the temperature range?

$A$ chemical reaction cannot occur at all if

Which of the following pairs of a chemical reaction is certain to result in a spontaneous reaction?

$A$ $4.50 \ g$ sample of methane occupies $12.7 \ L$ at $310 \ K$. Calculate the work done in $J$ when the gas undergoes isothermal expansion against a constant external pressure of $200 \ torr$ until the volume increases by $3.3 \ L$. (in $.99$)