Balance each of the following redox reactions occurring in
acidic aqueous solution.
art A
K(s)+Cr3+(aq)→Cr(s)+K+(aq)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
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Part B
Cd(s)+Cu+(aq)→Cd2+(aq)+Cu(s)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
Cd(s)+2Cu+(aq)→2Cu+(s)+Cd2+(aq)
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Part C
BrO−3(aq)+N2H4(g)→Br−(aq)+N2(g)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
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Use the half-reaction method to balance each redox reaction
occurring in acidic aqueous solution.
Part A
PbO2(s)+I−(aq)⟶Pb2+(aq)+I2(s)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
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Part B
SO32−(aq)+MnO4−(aq)→SO42−(aq)+Mn2+(aq)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
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Part C
S2O32−(aq)+Cl2(g)→SO42−(aq)+Cl−(aq)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
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Balance the following oxidation–reduction equation. The
reactions occur in a basic aqueous solution.
Cd2++ H 2S
→ Cd + S 8
S2- + F2 →
SO42- + F-
Cr + NO3- →
Cr(OH)4- +
NH3
MnO4- +
C2O42- →
MnO2 + CO2
Consider the following unbalanced redox reaction occurring in
acidic solution: H2SO3 (aq) + IO3-(aq) → SO42-(aq) + I2 (aq) a)
Balance the reaction. b) Using your table of standard reduction
potentials, calculate ΔG°rxn for this reaction.
Balance each redox reaction occurring in acidic aqueous
solution. Use the half-reaction method. Identify all phases in
answer
A) IO3-(aq)+SO2(g)------->
I2(s)+SO4^2-aq) B) Cr2O7^2- (aq) + Br-
(aq)-----------> Cr^3+(aq) + Br(aq)