# Problem: 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)

###### FREE Expert Solution

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:

88% (93 ratings) ###### Problem Details

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)