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 : 281
To calculate the cell potential (\(E_{\text{cell}}\)) for the electrochemical cell, we use the Nernst equation: \[ E_{\text{cell}} = E^\circ_{\text{cell}} - \frac{0.0591}{n} \log Q \] ### Step 1: Determine the Half-Reactions 1. Cadmium half-reaction: \[ \text{Cd}^{2+} + 2e^- \rightarrow \text{Cd}, \quad E^\circ = -0.40V \] 2. Chromium __________ ______ _________ ______ __________ _________ _________ __________.
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To calculate the cell potential (\(E_{\text{cell}}\)) for the electrochemical cell, we use the Nernst equation: \[ E_{\text{cell}} = E^\circ_{\text{cell}} - \frac{0.0591}{n} \log Q \] ### Step 1: Determine the Half-Reactions 1. Cadmium half-reaction: \[ \text{Cd}^{2+} + 2e^- \rightarrow \text{Cd}, \quad E^\circ = -0.40V \] 2. Chromium __________ ______ _________ ______ __________ _________ _________ __________.
_______ __________ ___ _______ ____ _______ ____ _____ ___.
_______ ___ ____ ________ _______.
___ _______ _____ __________ __________.
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