A certain reaction is known to have an activation energy E 78.0 kJ/mol. Furtherm

Question

A certain reaction is known to have an activation energy E 78.0 kJ/mol. Furthermore, the rate of this reaction is measured at 288. K and found to be 7.1 x10 M/s. Use this information to answer the questions in the table below. (You may need to use the scrollbar to see all the choices.) Suppose the concentrations of alll reactants is kept the same, but the temperature is raised by10% from 288, K to 3 17. K. The rate wil choose one How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is added, which has the effect of lowering the activation energy by 10%, from 78.0 kJ mol to 70.2 kJ/mol. How will the rate of the reaction change? The rate will choose one

Explanation / Answer

In case-1 when all reactants concentration remains same but temperature increases then the value of rate constant would increase as per Arrhenius equation(K=A.e-Ea/RT where Ea is activation energy and T is temperature). Hence the rate of reaction would also increase.

In case 2 when all reactants have same concentration and catalyst is added which reduces Ea then also the value of rate constant increases as per Arrhenius equation so the value of rate would also increase.

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