Coupled Reactions Practice Test

Two reactions are coupled in a metabolic sequence by sharing intermediate $M$ (Reaction 1 produces $M$, Reaction 2 consumes $M$). Reaction 1 is spontaneous: $L \rightarrow M$, $\Delta G = -40\ \text{kJ/mol}$. Reaction 2 is nonspontaneous: $M \rightarrow N$, $\Delta G = +12\ \text{kJ/mol}$. When coupled as $L \rightarrow N$, which condition allows the nonspontaneous reaction to proceed thermodynamically?

In a synthesis scheme, two reactions are coupled by sharing intermediate $E$. Reaction 1 is spontaneous: $D \rightarrow E$, $\Delta G = -2\ \text{kJ/mol}$. Reaction 2 is nonspontaneous: $E \rightarrow F$, $\Delta G = +9\ \text{kJ/mol}$. They are carried out together so the intended overall conversion is $D \rightarrow F$. Which statement is correct?