Subjects
| Sections | |||
|---|---|---|---|
| Redox Reaction | 32 mins | 0 completed | Learn Summary |
| Balancing Redox Reaction | 31 mins | 0 completed | Learn |
| The Nernst Equation | 11 mins | 0 completed | Learn |
| Faraday's Constant | 10 mins | 0 completed | Learn |
| Galvanic Cell | 85 mins | 0 completed | Learn |
| Batteries and Electricity | 9 mins | 0 completed | Learn |
| Additional Practice |
|---|
| Cell Notation |
| Standard Hydrogen Electrode |
| Cell Potential |
| Electroplating |
| Electrolysis of Water & Mixture of Ions |
| Additional Guides |
|---|
| Nernst Equation |
For the following electrochemical cell Cu(s) | Cu 2+ (aq, 0.0155M) || Ag+ (aq, 3.50M) | Ag(s)
Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K.
X(s) + Y4+(aq) ⇌ X4+(aq) + Y(s) K = 1.65 x 10 3
E° = ?V
Use the Nernst (Keq-Eocell) equation to determine Eocell of the reaction
Step 1. Determine the values and the working equation
Enter your friends' email addresses to invite them:
Join thousands of students and gain free access to 46 hours of Chemistry videos that follow the topics your textbook covers.