# Problem: 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

###### FREE Expert Solution

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

80% (150 ratings) ###### Problem Details

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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