Use standard reduction potentials to calculate the equilibri

Use standard reduction potentials to calculate the equilibrium constant at 25 C for decomposition of hydrogen peroxide.
2H2O2 (l) -> 2H20 (l) + O2 (g)

K=

Solution

Geez, You\'re both way off.

The answer is K= 3.45 *10^36

Here\'s how:

Equaton: ln[k]=nFEo/RT

Where n=#mol (of electrons transferred), F= Ferday\'s constant (96500 c/sec), Eo= cell potential, R=8.314J (ideal gas constant) and T=temp (Standard is 25C or 298K)

Eo= 1.08 (got by sum of reduction potential of products - sum of reduction potential of reactants) which is usually found in the appedix of your chem book.

So,

ln[k]=(2)(96500)(1.08)/ (8.314)(298)

ln[k]=84.1307

Take the e^ of both sides to cancel out ln

so e^84.1307= 3.45*10^36

Your answer.