In the decomposition of `H_2O_2` at 300 K, the energy of activation was found to be `18 kcal//"mol"` white it decreases to `6 kcal//"mol"` when the decomposition was carried out in the presence of a catalyst at 300 K.How many (Give you answer by multiplying `10^7`)

In the decomposition of `H_2O_2` at 300 K, the energy of activation wa

1.	In the decomposition of `H_2O_2` at 300 K, the energy of activation was found to be `18 kcal//"mol"` white it decreases to `6 kcal//"mol"` when the decomposition was carried out in the presence of a catalyst at 300 K.How many (Give you answer by multiplying `10^7`)
Answer» Correct Answer - 48 times Decomposition of `H_2O_2` order (Rxn)`H_2O_2toH_2OtoH_2O+1/2O_2` Then we know `K=Ae(-Ea)/(RT)` For uncatalysed Rxn `K_1=Ae(-Ea)/(RT) " " [T=300 K , R=2]` `K=Ae(-18xx10^3)/(2xx300)`..(i) and for catalysed Rxn `K_2=Ae(-6xx10^3)/(2xx300)`...(ii) Equation (2)/(1) `K_2/K_1=e((18-6)xx10^3)/(2xx300)` `K_2/K_1=e^20` `K_2/K_1=4.85xx10^8` Then catalysed reaction is `4.85xx10^8` times faster than uncatalysed Rxn.

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In the decomposition of `H_2O_2` at 300 K, the energy of activation was found to be `18 kcal//"mol"` white it decreases to `6 kcal//"mol"` when the decomposition was carried out in the presence of a catalyst at 300 K.How many (Give you answer by multiplying `10^7`)

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