The decomposition of hydrogen peroxide to form water and oxygen is represented b

Question

The decomposition of hydrogen peroxide to form water and oxygen is represented by the equation:

   2H2O2 (aq) 2H2O (l) + O2 (g) Hrxn = -195 kJ

- Determine the rate law for the reaction. Justify your response

b- Determine k , the rate constant, for the reaction. Include units

c- A proposed mechanism for the reaction is:

   H2O2 2HO

   H2O2 + HO H2O + HOO

   HOO + HO H2O + O2

Is this potentially a valid mechanism? Justify your response

Identify the slow step in the proposed mechanism?

Identify any intermediates or catalysts in the mechanism?

d- Will the reaction be spontaneous? Justify your response

e- “Increasing the temperature decreases the equilibrium constant but increases the rate of formation of O2(g)” Is this statement True or false? Justify your response

Explanation / Answer

H2O2 2HO (slow step)

   H2O2 + HO H2O + HOO (fast)

   HOO + HO H2O + O2   (fast)

Rate law

Rate= K[H2O2]

intermediates or catalysts HO and HOO

Rate constant K = sec-1 it is first order reaction.

e- “Increasing the temperature decreases the equilibrium constant but increases the rate of formation of O2(g)” Is this statement False.

It is exothermic reaction . Exothermic reaction takes place at low temperature.

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