Hello! I need help calculating the equilibrium constant for the redox reaction Sn(solid) + Zn2+(aqueous) ⇌ Sn2+(aqueous) + Zn(solid) Sn2+ ⇌ + 2e− Sn(solid) E° =−0.141 V Zn2+ ⇌ + 2e− Zn(solid) E° =−0.762 V My professor said the answer should be about 1.2 x 10-21, but I'm unsure how he came up with that value
Hello! I need help calculating the equilibrium constant for the redox reaction Sn(solid) + Zn2+(aqueous) ⇌ Sn2+(aqueous) + Zn(solid) Sn2+ ⇌ + 2e− Sn(solid) E° =−0.141 V Zn2+ ⇌ + 2e− Zn(solid) E° =−0.762 V My professor said the answer should be about 1.2 x 10-21, but I'm unsure how he came up with that value
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter13: Electrochemistry
Section: Chapter Questions
Problem 13.39PAE: Some calculators cannot display results of an antilog calculation if the power of 10 is greater than...
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Hello! I need help calculating the equilibrium constant for the
Sn2+ ⇌ + 2e− Sn(solid)
E° =−0.141 V
Zn2+ ⇌ + 2e− Zn(solid)
E° =−0.762 V
My professor said the answer should be about 1.2 x 10-21, but I'm unsure how he came up with that value
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