객관식
Which element is the best reducing agent?
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16. Oxidation and Reduction
Spontaneous Redox Reactions
객관식
Determine whether which of the following redox reactions will occur spontaneously in the forward direction?
a) Ni(s) + Zn2+(aq) → Ni2+(aq) + Zn(s)
b) Fe(s) + Pb4+(aq) → Fe2+(aq) + Pb(s)
c) Al(s) + Ag+(aq) → Al3+(aq) + Ag(s)
d) Pb(s) + Mn2+ (aq) → Pb2+(aq) + Mn(s)
A
Only b)
B
Both b) and c)
C
a), b) and c)
D
Both c) and d)
검증된 단계별 안내1
Identify the half-reactions for each redox reaction. For example, in reaction a), the oxidation half-reaction is Ni(s) → Ni²⁺(aq) + 2e⁻ and the reduction half-reaction is Zn²⁺(aq) + 2e⁻ → Zn(s).
Determine the standard reduction potentials (E°) for each half-reaction using a standard reduction potential table. The more positive the E° value, the greater the tendency for the species to be reduced.
Calculate the standard cell potential (E°cell) for each reaction by using the formula: E°cell = E°(reduction) - E°(oxidation).
Evaluate the spontaneity of each reaction. A positive E°cell indicates that the reaction is spontaneous in the forward direction.
Compare the calculated E°cell values for each reaction to determine which reactions are spontaneous. The reactions with positive E°cell values will occur spontaneously in the forward direction.
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