Calculate the work done in the following reaction at $27^{\circ} C$.
$4 SO_{2(g)} + 2 O_{2(g)} \rightarrow 4 SO_{3(g)}$
$(R = 8.314 \ J \ K^{-1} \ mol^{-1})$ (in $J$)

In the conversion of limestone to lime,$CaCO_{3(s)} \rightarrow CaO_{(s)} + CO_{2(g)}$,the values of $\Delta H^{\circ}$ and $\Delta S^{\circ}$ are $+179.1 \ kJ \ mol^{-1}$ and $160.2 \ J \ K^{-1} \ mol^{-1}$ respectively at $298 \ K$ and $1 \ bar$. Assuming that $\Delta H^{\circ}$ and $\Delta S^{\circ}$ do not change with temperature,the temperature above which the conversion of limestone to lime will be spontaneous is ........... $K$.

For a spontaneous reaction at all temperatures, which of the following is correct?

For a certain reaction,$\Delta H = -225 \ kJ \ mol^{-1}$ and $\Delta S = -150 \ J \ K^{-1} \ mol^{-1}$. Find the temperature at which $\Delta G$ is zero. (in $K$)

Under what conditions will a reaction become spontaneous at all temperatures?

When enthalpy and entropy change for a chemical reaction are $-2.5 \times 10^3 \ cal$ and $7.4 \ cal \ K^{-1}$ respectively,predict if the reaction at $298 \ K$ is: