Calculate the Eell for the cell reaction at 25 °C. Take note, not E°.el- 3 Zn (s) + 2 Cr²+ (aq) 3 Zn2+ (aq) + 2 Cr (s) The concentrations are [Cr*] = 0.010 M and [Zn2+] = 0.0085 M %3D The standard reduction potentials for Cr* and Zn+ are -0.74 V and -0.76 V, respectively. O0.02 V Do.0 v Oo.15 V O0.04 V
Calculate the Eell for the cell reaction at 25 °C. Take note, not E°.el- 3 Zn (s) + 2 Cr²+ (aq) 3 Zn2+ (aq) + 2 Cr (s) The concentrations are [Cr*] = 0.010 M and [Zn2+] = 0.0085 M %3D The standard reduction potentials for Cr* and Zn+ are -0.74 V and -0.76 V, respectively. O0.02 V Do.0 v Oo.15 V O0.04 V
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.69QE: What is the voltage of a concentration cell of Fe2+ ions where the concentrations are 0.0025 and...
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![Calculate the E-n for the cell reaction at 25 °C. Take note, not E°..
cell-
3 Zn (s) + 2 Cr²* (aq) → 3 Zn²* (aq) + 2 Cr (s)
The concentrations are [Cr*] = 0.010 M and [Zn2+] = 0.0085 M
The standard reduction potentials for Cr** and Zn2* are -0.74 V and -0.76 V, respectively.
Oo.02 v
Oo.0 v
D0.15 v
Oo.04 V](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff70653cf-152a-4edf-8c62-be28491f21e3%2F0702c5be-e805-4ee7-8a0b-0e7abd05c9ec%2Fuclnp7r_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Calculate the E-n for the cell reaction at 25 °C. Take note, not E°..
cell-
3 Zn (s) + 2 Cr²* (aq) → 3 Zn²* (aq) + 2 Cr (s)
The concentrations are [Cr*] = 0.010 M and [Zn2+] = 0.0085 M
The standard reduction potentials for Cr** and Zn2* are -0.74 V and -0.76 V, respectively.
Oo.02 v
Oo.0 v
D0.15 v
Oo.04 V
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