Chemistry, asked by Aadill3245, 10 months ago

The rate of a reaction depends upon the temperature and is quantitatively expressed as
k= Ae ⁻Eₐ/RT
I) If a graph is plotted between log k and 1/T, write the expression for the slope of the reaction?
ii) If at under different conditions Ea1 and Ea2 are the activation energy of two reactions If Ea1 = 40 J / mol and Ea2 = 80 J / mol. Which of the two has a larger value of the rate constant?

Answers

Answered by msophias77

Answer:

Rate constant is inversely proportional to activation energy by Arrhenius equation

Explanation: So, k1 > k2

Answered by Anonymous

The answers about enzyme kinetics are written below-

1. On doing log of both the sides, of the equation provided, the resulting equation will be-

Log k = log A - Ea/RT

When graph is plotted between log K and 1/T, according to the formula -

Y = mx + c, slope will be - -Ea/R

In the equation, k represents rate constant, A represents pre exponential factor, Ea is for activation energy, R refers to gas constant and T is temperature.

2. As seen from the above equation, more the activation energy less will be the rate constant. Hence, Ea1 will have greater value of rate constant in comparison to Ea2.

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