Question

From standard reduction potentials, calculate the equilibrium constant at 25 ∘c for the reaction 2mno−4(aq)+10cl−(aq)+16h+(aq)→2mn2+(aq)+5cl2(g)+8h2o(l)

Answer 1

To calculate the equilibrium constant at 25°C for the given reaction, use the information from the standard reduction potentials given in the question. Write the half-reactions and use the Nernst equation to calculate the cell potential. Then, calculate the equilibrium constant using the relation ΔG = -RTlnK.

Step-by-step explanation:

To calculate the equilibrium constant at 25°C for the given reaction, we need to use the information from the standard reduction potentials given in the question. We can first write the half-reactions for the species involved in the reaction:

1. 
   
3. 2MnO4-(aq) + 16H+(aq) + 10e- → 2Mn2+(aq) + 8H2O(l)
4. 
   
6. 10Cl-(aq) → 5Cl2(g) + 10e-

Then, we can use the Nernst equation to calculate the cell potential for the reaction:

Nernst equation:

E = E0 - (0.0592/n) * log(Q)

Where:

• 
  
• E is the cell potential
• 
  
• E0 is the standard cell potential
• 
  
• n is the number of electrons transferred in the balanced equation
• 
  
• Q is the reaction quotient, which can be calculated using the concentrations of the species involved

By calculating the cell potential and using the equation ΔG = -nFEcell, where ΔG is the change in Gibbs free energy, F is Faraday's constant, and Ecell is the cell potential, we can then calculate the equilibrium constant K using the relation ΔG = -RTlnK.

By substituting the values into the equations and calculating, we can find the equilibrium constant for the given reaction at 25°C.