Question

In which of the following reactions, standard entropy change (ΔS°) is positive and standard Gibb’s energy change (ΔG°) decreases sharply with increase in temperature ?
(a) $C (graphite) + \frac{1}{2}O_2(g) \rightarrow CO(g)$
(b) $CO(g) + \frac{1}{2}O_2(g) \rightarrow CO_2(g)$
(c) $Mg(s) + \frac{1}{2}O_2(g) \rightarrow MgO(s)$
(d) $\frac{1}{2}C (graphite) + \frac{1}{2}O_2(g) \rightarrow \frac{1}{2}CO_2(g)$

Answer 1

D) 1/2 C (graphite) +1/2 O2 (g) → 1/2 CO2 (g)

This Reaction Has a Positive Entropy And It's Free Energy Decreases with Increase in Temp.

Answer 2

Answer:

D

Explanation:

The change in gaseous moles Δn

g must be highest which indicates the more gaseous product is formed which increases randomness and thus entropy increases.