Consider the following balanced redox reaction: H2SO3 (aq) + 2 Mn (s) + 4 H+ (aq) → S (s) + 2 Mn2+ (aq) + 3 H2O (l) Which element was oxidized during this reaction?

For this question, answer it on your work paper. In the box below, type “complete” when finished. Make sure to show all of your work Consider the voltaic cell constructed using the following reaction: Ni (s) + Pb2+ (aq) → Ni2+ (aq) + Pb (s) Calculate the cell potential (Ecell) when = 1.87 M and = 0.420 M

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Consider the following balanced redox reaction: H2SO3 (aq) + 2 Mn (s) + 4 H+ (aq) → S (s) + 2 Mn2+ (aq) + 3 H2O (l) Which element was reduced during this reaction?

For this question, answer it on your work paper. In the box below, type “complete” when finished. Make sure to show all of your work A 0.125-M solution of Mn(NO3)2 is saturated with H2S ( = 0.10 M). At what pH does MnS begin to precipitate? MnS(s) ⇌ Mn2+(aq) + S2−(aq)                                 Ksp=4.3×10−22 H2S(aq) + 2H2O(l)  ⇌ 2H3O+(aq) + S2−(aq)                K=1.0×10−26

Iodine is the reducing agent in the following balanced redox reaction: I2 (s) + 5 Cu2+ (aq) + 6 H2O (l) → 2 IO3- (aq) + 5 Cu (s) + 12 H+ (aq)

For this question, answer it on your work paper. In the box below, type “complete” when finished. Make sure to show all of your work Consider the voltaic cell that uses the following reaction: Zn (s) + Pb2+ (aq) → Zn2+ (aq) + Pb (s) Calculate the cell potential (Ecell) when = 2.54 M and = 0.157 M

Iodine is the reducing agent in the following balanced redox reaction: I2 (s) + 5 Cu2+ (aq) + 6 H2O (l) → 2 IO3- (aq) + 5 Cu (s) + 12 H+ (aq)

Consider the following balanced redox reaction: Cr2O72- (aq) + 6 I- (aq) + 14 H+ (aq) → 2 Cr3+ (aq) + 3 I2 (s) + 7 H2O (l) Which element was reduced during this reaction?

Using the standard reduction potentials document, calculate the cell potential at 25 °C for the following voltaic cell: Cd (s) | Cd2+ (aq) || Sn2+ (aq) | Sn (s)