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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: yoyohs on December 08, 2021, 02:29:15 PM

Title: Galvanic cell question, urgent
Post by: yoyohs on December 08, 2021, 02:29:15 PM

A voltaic cell at 25^oC consists of Mn/Mn²⁺ and Cd/Cd²⁺ half-cells with the initial concentrations [Mn²⁺] = 0.100 M and [Cd²⁺] = 0.0100 M. Use the Nernst equation to calculate E for this cell.
Cd⁺²(aq) + 2e- = Cd(s) . . . . . . E^o = -0.40 V
Mn⁺²(aq) + 2e- = Mn(s) . . . . . . . E^o = -1.18 V

this is what i did, but it is wrong. https://drive.google.com/file/d/1HzBRnAl7CzwAbmwGWjE0z1JWF1M2sypu/view?usp=sharing (https://drive.google.com/file/d/1HzBRnAl7CzwAbmwGWjE0z1JWF1M2sypu/view?usp=sharing)

Title: Re: Galvanic cell question, urgent
Post by: mjc123 on December 09, 2021, 05:45:40 AM

Write the equation for the spontaneous cell reaction. What is Q?
(Alternatively, work out the modified potentials for each electrode separately, and then combine them.)