Question

Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: $Cu^{2+}(aq) + Zn(s) \rightarrow Cu(s) + Zn^{2+}(aq)$ Suppose the cell is prepared with 1.36 $M$ $Cu^{2+}$ in one half-cell and 4.64 $M$ $Zn^{2+}$ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

Name: using the nernst equation to calculate nonstandard cell voltage a galvanic cell at a temperature of 250 c is powered by the following redox reaction cu2aq zns rightarrow cus zn2aq suppose th 96171
Uploaded: 2022-07-06T16:49:45-08:00
Duration: 2 min 46 s
Channel: Shaiju T
Description: using the nernst equation to calculate nonstandard cell voltage a galvanic cell at a temperature of 250 c is powered by the following redox reaction cu2aq zns rightarrow cus zn2aq suppose th 96171

          Using the Nernst equation to calculate nonstandard cell voltage
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction:
$Cu^{2+}(aq) + Zn(s) \rightarrow Cu(s) + Zn^{2+}(aq)$
Suppose the cell is prepared with 1.36 $M$ $Cu^{2+}$ in one half-cell and 4.64 $M$ $Zn^{2+}$ in the other.
Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

using the nernst equation to calculate nonstandard cell voltage a galvanic cell at a temperature of 250 c is powered by the following redox reaction cu2aq zns rightarrow cus zn2aq suppose th 96171

Added by Stephanie B.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Shaiju T

07/06/2022

Step 1

314 J/(mol·K)) T is the temperature in Kelvin n is the number of moles of electrons transferred in the balanced redox reaction F is the Faraday constant (96485 C/mol) Q is the reaction quotient Show more…

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Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: $Cu^{2+}(aq) + Zn(s) \rightarrow Cu(s) + Zn^{2+}(aq)$ Suppose the cell is prepared with 1.36 $M$ $Cu^{2+}$ in one half-cell and 4.64 $M$ $Zn^{2+}$ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.