We are asked to calculate for the standard potential (E°cell) of the reaction. We will use the Nernst Equation to calculate for the ratio. The Nernst Equation relates the concentrations of compounds and cell potential.
E°cell = cell potential, V
R = gas constant = 8.314 J/(mol·K)
T = temperature, K
n = mole e- transferred
F = Faraday’s constant, 96485 C/mol e-
K = equilibrium constant
Let’s first determine how many electrons were transferred in the reaction:
Calculate the cell potential for the following reaction when the pressure of the oxygen gas is 2.50 atm, the hydrogen ion concentration is 0.10 mol/L, and the bromide ion concentration is 0.25 mol/L.
O2(g) + 4H+(aq) + 4Br -(aq) → 2H2O(l) + 2Br2(l)
Frequently Asked Questions
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 The Nernst Equation concept. You can view video lessons to learn The Nernst Equation. Or if you need more The Nernst Equation practice, you can also practice The Nernst Equation practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Lapeyrouse's class at UCF.