The reaction N2(g) + 3 H2(g) → 2 NH3(g), does not favor formation of products at room temperature but does favor formation of products at a much higher temperature. What can you conclude from this about the signs of ∆H° and ∆S°, assuming that the enthalpy and entropy changes are not greatly affected by the temperature change? a. ∆H° must be negative.
b. ∆S° must be equal to zero.
c. ∆H° must be equal to zero.
d. ∆H° must be positive.
e. ∆S° must be negative.
f. ∆S° must be positive.