What is E°cell (in V) for a redox reaction that has ΔrG° = 164 kJ mol-1 at 25°C ? Assume 4 electrons are transferred in the balanced redox reaction.If needed, F = 96485 C/mol.Answer:Question 4
Question
What is E°cell (in V) for a redox reaction that has ΔrG° = 164 kJ mol-1 at 25°C ? Assume 4 electrons are transferred in the balanced redox reaction.If needed, F = 96485 C/mol.Answer:Question 4
Solution
To calculate the E°cell, we can use the formula ΔrG° = -nFE°cell.
Given: ΔrG° = 164 kJ mol-1 = 164000 J mol-1 (since 1 kJ = 1000 J) n = 4 (number of electrons transferred) F = 96485 C/mol (Faraday's constant)
We can rearrange the formula to solve for E°cell:
E°cell = -ΔrG° / nF
Substituting the given values:
E°cell = -(-164000 J mol-1) / (4 * 96485 C/mol)
E°cell = 0.426 V
So, the E°cell for the redox reaction is 0.426 V.
Similar Questions
What is the E°cell (in V) for a redox reaction that has equilibrium constant K =3.6 x 1012 at 25°C ? Assume 1 electrons are transferred in the balanced redox reaction. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4".Answer:Question 5
. For the reaction below at standard conditions, what would be DG° ?2Al(s) + 3Mn2+(aq) → 2Al3+(aq) + 3Mn(s) ; E° cell = 0.49 V-284000 kJ-284 kJ-142 kJ-142,000 kJ
Calculate ΔG° for the reaction below under standard conditions at 25°C. 2S(s) + 3O2(g) + 2H2O(l) → 2H2SO4(l) ΔH° = -1056 kJ/molΔS° = -505 J/molHint: Pay attention to units of ΔH° and ΔS°
For the reaction below at standard conditions, what would be K?2Ag+(aq) + Cd(s) → Cd2+(aq) + 2Ag(s) ; E°cell = 1.20 V3.9 × 10402.0 × 10202.4 × 10441.6 × 1022
Calculate the ΔG for the cell reaction at 298 K for the cell.Zn(s) | Zn2+ || Cd2+ | Cd(s)Given : F = 96500 C mol–1, Ecell = 0.44 V
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.