We’re being asked to determine the electromotive force (EMF) or standard cell potential (E°cell) of the reaction occurring in an electrochemical cell. To calculate for the standard cell potential, use the following equation:
When a balanced reaction is given, identify the anode and the cathode half-reactions by determining the changes in oxidation states of each species based on the given reaction:
A voltaic cell utilizes the following reaction and operates at 298 K:
3Ce4 + (aq) + Cr(s) → 3Ce3 + (aq) + Cr3 + (aq).
What is the emf of this cell under standard conditions?
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Cell Potential concept. If you need more Cell Potential practice, you can also practice Cell Potential practice problems.
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Based on our data, we think this problem is relevant for Professor Stec's class at UIC.