Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn 2+ and a nickel electrode immersed in 0.10 M Ni 2+ . Zn 2+ + 2e- $\to$ Zn $\varepsilon$° = -0.76 V Ni 2+ + 2e- $\to$ Ni $\varepsilon$° = -0.23 V -Calculate $\varepsilon$ at 25°C for the cell shown below,given the following data: K sp for AgCl = 1.6 $\times$10 - 10

The Answer of Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn 2+ and a nickel electrode immersed in 0.10 M Ni 2+ . Zn 2+ + 2e- $\to$ Zn $\varepsilon$° = -0.76 V Ni 2+ + 2e- $\to$ Ni $\varepsilon$° = -0.23 V -Calculate $\varepsilon$ at 25°C for the cell shown below,given the following data: K sp for AgCl = 1.6 $\times$10 - 10

Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn 2+ and a nickel electrode immersed in 0.10 M Ni 2+ . Zn 2+ + 2e- $\to$ Zn $\varepsilon$° = -0.76 V Ni 2+ + 2e- $\to$ Ni $\varepsilon$° = -0.23 V -Calculate $\varepsilon$ at 25°C for the cell shown below,given the following data: K sp for AgCl = 1.6 $\times$10 - 10

The Answer of Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn 2+ and a nickel electrode immersed in 0.10 M Ni 2+ . Zn 2+ + 2e- $\to$ Zn $\varepsilon$° = -0.76 V Ni 2+ + 2e- $\to$ Ni $\varepsilon$° = -0.23 V -Calculate $\varepsilon$ at 25°C for the cell shown below,given the following data: K sp for AgCl = 1.6 $\times$10 - 10

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Consider an Electrochemical Cell with a Zinc Electrode Immersed in 1.0

Question 77

Multiple Choice

Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn²⁺ and a nickel electrode immersed in 0.10 M Ni²⁺.
Zn²⁺ + 2e- $\to$ Zn
$\varepsilon$ ° = -0.76 V
Ni²⁺ + 2e- $\to$ Ni
$\varepsilon$ ° = -0.23 V
-Calculate $\varepsilon$ at 25°C for the cell shown below,given the following data: $Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2+ and a nickel electrode immersed in 0.10 M Ni2+. Zn2+ + 2e- \to Zn \varepsilon ° = -0.76 V Ni2+ + 2e- \to Ni \varepsilon ° = -0.23 V -Calculate \varepsilon at 25°C for the cell shown below,given the following data: Ksp for AgCl = 1.6 \times 10-10 A) 0.83 V B) 0.54 V C) 1.01 V D) 2.98 V E) cannot be determined from the data given$
$Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2+ and a nickel electrode immersed in 0.10 M Ni2+. Zn2+ + 2e- \to Zn \varepsilon ° = -0.76 V Ni2+ + 2e- \to Ni \varepsilon ° = -0.23 V -Calculate \varepsilon at 25°C for the cell shown below,given the following data: Ksp for AgCl = 1.6 \times 10-10 A) 0.83 V B) 0.54 V C) 1.01 V D) 2.98 V E) cannot be determined from the data given$
$Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2+ and a nickel electrode immersed in 0.10 M Ni2+. Zn2+ + 2e- \to Zn \varepsilon ° = -0.76 V Ni2+ + 2e- \to Ni \varepsilon ° = -0.23 V -Calculate \varepsilon at 25°C for the cell shown below,given the following data: Ksp for AgCl = 1.6 \times 10-10 A) 0.83 V B) 0.54 V C) 1.01 V D) 2.98 V E) cannot be determined from the data given$
$Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2+ and a nickel electrode immersed in 0.10 M Ni2+. Zn2+ + 2e- \to Zn \varepsilon ° = -0.76 V Ni2+ + 2e- \to Ni \varepsilon ° = -0.23 V -Calculate \varepsilon at 25°C for the cell shown below,given the following data: Ksp for AgCl = 1.6 \times 10-10 A) 0.83 V B) 0.54 V C) 1.01 V D) 2.98 V E) cannot be determined from the data given$ $Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2+ and a nickel electrode immersed in 0.10 M Ni2+. Zn2+ + 2e- \to Zn \varepsilon ° = -0.76 V Ni2+ + 2e- \to Ni \varepsilon ° = -0.23 V -Calculate \varepsilon at 25°C for the cell shown below,given the following data: Ksp for AgCl = 1.6 \times 10-10 A) 0.83 V B) 0.54 V C) 1.01 V D) 2.98 V E) cannot be determined from the data given$
K_sp for AgCl = 1.6 $\times$ 10^-¹⁰

A) 0.83 V
B) 0.54 V
C) 1.01 V
D) 2.98 V
E) cannot be determined from the data given

Correct Answer:

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