Chapter 9, Problem 9.146MP

For a process to be spontaneous, the total entropy of the system and its surroundings must increase; that is $\Delta S_{\text{total}}=\Delta S_{\text{system}}=\Delta S_{\text{surr}}>0$ for a spontaneous process
Furthermore, the entropy change in the surroundings, $\Delta S_{\text{surr}}$ is related to the enthalpy change for the process by the equation $\Delta S_{\text{surr}}=\Delta H/T.$
(a) Since both $\Delta G$ and $\Delta S_{\text{total}}$ offer criteria for spontaneity, they must be related. Derive a relationship between them.
(b) What is the value of $\Delta S_{\text{surr}}$ for the photosynthesis of glucose from CO₂ at 298 K?
$6C{O}_2\left(g\right)+6H_{2}O\left(l\right)\to C_6{H}_{12}{O}_6\left(s\right)+6O_2\left(g\right)$
$\begin{array}{l}\Delta G°=287\text{9 kJ}\\ \Delta S°=-262\text{ J/k}\end{array}$