Question
What is the cell potential of an electrochemical cell made of a cadmium electrode in a 0.1 M Cd(NO3)2 solution and chromium electrode in a 1 x 10 M Cr(NO3)3 solution.
[Given: ]
Answer :
Word Count : 264
To calculate the cell potential (\(E_{\text{cell}}\)) for the electrochemical cell made of a cadmium (Cd) electrode and a chromium (Cr) electrode, we use the Nernst equation: \[ E_{\text{cell}} = E_{\text{cell}}^{0} - \frac{0.0591}{n} \log Q \] ### Step 1: Identify Half-Reactions and Standard Reduction Potentials The given standard reduction potentials are: \[ E_{\text{Cd}^{2+}/\text{Cd}}^{0} _______ ____ _________ ______ ___ ___ _______.
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To calculate the cell potential (\(E_{\text{cell}}\)) for the electrochemical cell made of a cadmium (Cd) electrode and a chromium (Cr) electrode, we use the Nernst equation: \[ E_{\text{cell}} = E_{\text{cell}}^{0} - \frac{0.0591}{n} \log Q \] ### Step 1: Identify Half-Reactions and Standard Reduction Potentials The given standard reduction potentials are: \[ E_{\text{Cd}^{2+}/\text{Cd}}^{0} _______ ____ _________ ______ ___ ___ _______.
_____ _____ _______ ___ __________ __________ ______ ____ ________ _________ ________.
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