Recall that if:
• ΔG < 0 or ΔG = (–); the reaction is spontaneous
• ΔG = 0; the reaction is at equilibrium
• ΔG > 0 or ΔG = (+); the reaction is non-spontaneous
Which of the following reactions are spontaneous (favorable)?
A. 2Mg(s )+ O2(g) → 2MgO (s) Δ G = - 1137 kJ / mol
B. NH3(g)+ HCl(g ) → NH4 Cl(s) Δ G = - 91.1 kJ / mol
C. AgCl(s) → Ag+ (aq) + Cl-[aq) Δ G = 55.6 kJ / mol
D. 2H2(g)+ O2(g) → 2H2O(g) Δ G = 456 kJ / mol
E. C(s)+H2O(t) → CO(g)+H2(g) Δ G = 90.8 kJ / mol
F. CH4(g) + 2O2(g) → CO2(g)+2H2O(l) Δ G = -820 kJ / mol
Check all spontaneous reactions.
a) Reaction A
b) Reaction B
c) Reaction C
d) Reaction D
e) Reaction E
f) Reaction F
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