Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Ag H+ ←H₂(g) Standard reduction potentials: 2H+2e →→→→ H₂ Eº = 0 V Ag+ leAg Eº=0.800 V
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Ag H+ ←H₂(g) Standard reduction potentials: 2H+2e →→→→ H₂ Eº = 0 V Ag+ leAg Eº=0.800 V
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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.140QP
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Question
![Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell
is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C.
Ag Ag+
+H
Standard reduction potentials:
2H+ + 2e¯ → H₂ Eº = 0 V
Ag+le
- H₂(g)
←
→ Ag E°=0.800 V](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa02a222c-09b7-48e2-8f10-299d6aeba7af%2F2fcbc81e-f5c8-4e76-84bc-be699de84b35%2Fwdg6u9_processed.png&w=3840&q=75)
Transcribed Image Text:Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell
is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C.
Ag Ag+
+H
Standard reduction potentials:
2H+ + 2e¯ → H₂ Eº = 0 V
Ag+le
- H₂(g)
←
→ Ag E°=0.800 V
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