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What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F, pressure is 5.95×10-4 atm, the F- concentration is 1.35M, and the Pb²+ concentration is 1.23M ? F2(g) + Pb(s)- →2F°(aq) + Pb²*(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F, pressure is 5.95×10-4 atm, the F- concentration is 1.35M, and the Pb²+ concentration is 1.23M ? F2(g) + Pb(s)- →2F°(aq) + Pb²*(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 5.95×10-4 atm, the F¯ concentration is 1.35M, and the Pb²+ concentration is 1.23M ? F2(g) + Pb(s) 2F (aq) + Pb2*(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
Transcribed Image Text:What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 5.95×10-4 atm, the F¯ concentration is 1.35M, and the Pb²+ concentration is 1.23M ? F2(g) + Pb(s) 2F (aq) + Pb2*(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
Expert Solution
Step 1

Given reaction is : 

F2 (g) + Pb (s) -------> 2F- (aq) + Pb2+ (aq) 

Pressure of F2 = PF2 = 5.95 x 10-4 atm 

Molar concentration of F- = [F-] = 1.35 M 

Molar concentration of Pb2+ = [Pb2+] = 1.23 M 

Standard cell potential = E0cell = ? 

The cell reaction given is spontaneous for the given concentration or not = ?

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