Question

How does catalyst make Hydrogen Peroxide’s decomposition quicker?

Answer 1

Hydrogen peroxide is thermodynamically unsteady and deteriorates to shape water and oxygen with a $\Delta$ Ho of $-2884.5kJ/kg\left[ {33} \right]$ and $\Delta$ S of $70.5J/\left( {mol\cdot} \right):$

Complete step by step answer:
A catalyst makes the decay response of hydrogen peroxide quicker in light of the fact that it furnishes an elective pathway with a lower activation energy for the response to take. Enactment energy is only a term used to communicate the base energy needed all together for a response to happen.
On the off chance that no catalyst is there it will require some investment to finish the disintegration of hydrogen peroxide
At the point when a catalyst is added, an elective pathway through which the reaction can shape water and Oxygen gas is presented. The speed of a catalysed reaction will increment since this elective pathway has a lower enactment energy. This is what an elective pathway implies. For instance, suppose you add potassium iodide, $KI$ , to a hydrogen peroxide solution.
Potassium iodide will separate totally to give potassium particles, ${K^ + },$ and iodide particles, ${I^ - }.$ The disintegration reaction will presently occur in two stages.

{\left( 1 \right):O2 + {I^ - } \to O{I^ - } + H2O} \\\ {\left( 2 \right):{\text{ }}H2O2 + O{I^ - } \to H2O + O2 + {I^ - }} \end{array}$$ An iodide ion will react with a hydrogen peroxide to produce water and hypoiodite ion $$O{I^ - }$$ . Then, a hypoiodite ion will react with another hydrogen peroxide molecule to produce water, oxygen gas, and iodine. That's why a catalyst is never consumed in a reaction - it is reformed at the end of the multi-step reaction. Adding equations (1) and (2) together will get the overall reaction $$2H2O + {I^ - } + O{I^ - } \to O{I^ - } + 2{H_2}O + {O_2} + {I^ - }$$ **Note:** 1.The type of reaction with hydrogen peroxide in presence of catalyst is exothermic and gas evolution. 2.always wear protective equipment while performing any exothermic reaction