Question

Hydrogen peroxide decomposes into water and oxygen by thefollowing reaction:

2 H2O2(aq) ↔ 2 H2O(l) + O2(g) ΔHrxn = -94.64 kJ/mol

Experimental evidence tells us that this reaction is first orderwith respect to hydrogen peroxide, with an activation energy of75.3 kJ/mol at 300 K.
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a)What is the activation energy for the reverse reaction?

b)Sketch the reaction pathway below. Be sure to label the axes,reactants, products, transition state, and energies.

c)Assuming the forward and reverse reaction have the same frequencyfactor, what is the equilibrium constant for this reaction?(when you answer this question,you will need to write down the value for K, and the temperaturethat you calculated K at.)

d)Catalase is an enzyme found in nearly all living organisms thatcatalyzes the hydrogen peroxide decomposition reaction shown aboveby lowering the activation energy of the forward reaction to 8.8kJ/mol. How many times faster does hydrogen peroxide decompose inthe presence of catalase?

e)What temperature would we need to decompose hydrogen peroxode atto achieve the same rate increase achieved with catalase?

I have the answers for a) and b) Ineed the answers for c), d), & e). I split them up because Ithought it was too long of a question so I can offer more points.Thanks.

Answer for a) and b):

(a) ΔH of reverse reaction = -ΔH offorward reaction

= -(-94.64 kJ/mol) = +94.64kJ/mol

Activation energy of reversereaction

= activation energy of forwardreaction + ΔH of reverse reaction

= 75.3 + 94.64 = 169.94kJ/mol

(b) The forward reaction isexothermic, and the reaction pathway is shown below: