For the following reaction that occurs at 25°C. 3Zn(s) + 2Cr"(aq) 3Zn2*(aq) + 2Cr(s) (a) Write the cell notation. (b) Calculate the standard electrode potential, E°cell. Calculate the cell potential if the concentrations of Cr3+ and Zn2+ ions are 0.10 M and 0.0090 M respectively. (c) (d) Calculate the equilibrium constant for the reaction: 3Zn(s) + 2Cr3*(aq) = 3Zn2"(aq) + 2Cr(s) [+0.02 V, +0.06 V, 1.1x10²]
For the following reaction that occurs at 25°C. 3Zn(s) + 2Cr"(aq) 3Zn2*(aq) + 2Cr(s) (a) Write the cell notation. (b) Calculate the standard electrode potential, E°cell. Calculate the cell potential if the concentrations of Cr3+ and Zn2+ ions are 0.10 M and 0.0090 M respectively. (c) (d) Calculate the equilibrium constant for the reaction: 3Zn(s) + 2Cr3*(aq) = 3Zn2"(aq) + 2Cr(s) [+0.02 V, +0.06 V, 1.1x10²]
Chemistry
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ISBN:9781305957404
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Chapter1: Chemical Foundations
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![12.
For the following reaction that occurs at 25°C.
3Zn(s) + 2Cr3*(aq) 3Zn2*(aq) + 2Cr(s)
(a)
Write the cell notation.
(b)
Calculate the standard electrode potential, E°cell.
Calculate the cell potential if the concentrations of Cr3+ and Zn2+ ions are 0.10
M and 0.0090 M respectively.
(c)
(d)
Calculate the equilibrium constant for the reaction:
3Zn(s) + 2Cr3"(aq) 3Zn2*(aq) + 2Cr(s)
[+0.02 V, +0.06 V, 1.1×10²]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F92c5294f-230f-469d-810f-0bd983494e34%2Fe4970e5b-de57-4861-9d56-f4c07b760375%2Fchfz5f_processed.jpeg&w=3840&q=75)
Transcribed Image Text:12.
For the following reaction that occurs at 25°C.
3Zn(s) + 2Cr3*(aq) 3Zn2*(aq) + 2Cr(s)
(a)
Write the cell notation.
(b)
Calculate the standard electrode potential, E°cell.
Calculate the cell potential if the concentrations of Cr3+ and Zn2+ ions are 0.10
M and 0.0090 M respectively.
(c)
(d)
Calculate the equilibrium constant for the reaction:
3Zn(s) + 2Cr3"(aq) 3Zn2*(aq) + 2Cr(s)
[+0.02 V, +0.06 V, 1.1×10²]
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