Multiple Choice
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 2 5°C. (The equation is balanced.) Pb(s) + Br2(l) → Pb2+(aq) + 2 Br⁻(aq)
Pb2+(aq) + 2 e⁻ → Pb(s) E° = -0.13 V
Br2(l) + 2 e⁻ → 2 Br⁻(aq) E° = +1.07 V
A) +1.20 V
B) +0.94 V
C) -0.94 V
D) -1.20 V
E) -0.60 V
Correct Answer:
Verified
Correct Answer:
Verified
Q40: Which of the following is the weakest
Q42: Use the standard half-cell potentials listed below
Q43: Describe how water can be made to
Q44: Calculate the cell potential for the following
Q46: Determine the redox reaction represented by the
Q47: Which of the following is the strongest
Q48: A galvanic cell consists of a Zn<sup>2+</sup>/
Q48: Explain the significance of the standard hydrogen
Q98: Identify the battery that is in most
Q129: Use the standard half-cell potentials listed below