Question

What is true about this reaction?

2 Na (s) + 1 Cl2 (g) --> 2 NaCl (s) at 25 degrees Celsius and 1 atmosphere

A) The reaction produces no change in G (change in free energy)
B) The reaction is non-spontaneous
C) The reaction is spontaneous
D) The reaction produces a positive change in free energy (G)

Is it B?

Answer 1

\[\Large \Delta G = \Delta H - T \Delta H\]
We have an exothermic reaction here.
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-When ΔG is positive, the process proceeds spontaneously in reverse.
-When ΔG is zero, the process is already in equilibrium, with no net change taking place over time.
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-When ΔS is positive and ΔH is negative, a process is always spontaneous
-When ΔS is negative and ΔH is negative, a process is spontaneous at low temperatures, where exothermicity is important.
+When ΔS is negative and ΔH is positive, a process is not spontaneous at any temperature, but the reverse process is spontaneous.
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Since ΔH is negative here, because its exothermic reaction, then the process is spontaneous.
We now confirm that A, B and D is not the answer.

Answer 2

thank you so much!