Based on the half-reactions and their respective standard reduction potentials below, what is the standard cell potential for the reaction that is expected to occur?
Fe3+(aq) + e- → Fe2+(aq) 0.77 V
Sn4+(aq) + 2 e- → Sn2+(aq) 0.15 V
Pb2+(aq) + 2 e- → Pb(s) -0.13 V
ANSWER:
Based on the half-reactions and their respective standard reduction potentials below, what is the standard cell potential for the reaction that is expected to occur?
Fe3+(aq) + e- → Fe2+(aq) 0.77 V
Sn4+(aq) + 2 e- → Sn2+(aq) 0.15 V
Pb2+(aq) + 2 e- → Pb(s) -0.13 V
Answers:
0.64 V
0.90 V
0.28 V
1.03 V
i dont know where too begin
Same mixed up question as the next one. See my comments there.
To determine the standard cell potential for the reaction that is expected to occur, you can use the Nernst equation. The Nernst equation relates the standard cell potential (E°), the actual cell potential (E), the reaction quotient (Q), the Faraday constant (F), the gas constant (R), and the temperature (T).
The formula for the Nernst equation is:
E = E° - (RT / nF) * ln(Q)
In this case, we need to determine the standard cell potential (E°) based on the given half-reactions and their respective reduction potentials. To do this, we need to add the half-reactions together and adjust the coefficients to balance electrons.
The balanced equation for the overall reaction is:
3 Fe3+(aq) + Sn4+(aq) + 2 Pb2+(aq) → 3 Fe2+(aq) + Sn2+(aq) + 2 Pb(s)
The total number of electrons transferred in the balanced equation is 3 * 1 + 2 * 2 = 7.
Now we can calculate the standard cell potential (E°) using the reduction potentials given:
E°cell = E°cathode - E°anode
For the cathode: Fe3+(aq) + e- → Fe2+(aq) (E° = 0.77 V)
For the anode: Sn4+(aq) + 2 e- → Sn2+(aq) (E° = 0.15 V)
E°cell = 0.15 V - 0.77 V
E°cell = -0.62 V
The standard cell potential (E°cell) for the reaction that is expected to occur is -0.62 V.
Therefore, none of the given answer choices (0.64 V, 0.90 V, 0.28 V, 1.03 V) are correct. The correct answer is -0.62 V.