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For the reaction A(g) + B(g) → AB(g), the rate is 0.20 mol/L . s , when [A]₀ = [B]₀ = 1.0 mol/L. If the reaction is first order in B and second order in A, what is the rate when [A]₀ = 2.0 mol/L and [B]₀ = 3.0 mol/L?



Answer :

mahima6824soni

The rate of the reaction when  [A]₀ = 2.0 mol/L and [B]₀ = 3.0 mol/L is 2.4 mol/L xs.

What is the rate of the reaction?

The rate of the reaction is the speed of the reaction. It is the speed of the reaction that happens in a time.

R = k [A]² [B]³

Given that

The reaction is A(g) + B(g) → AB(g)

[A] initial = [B] initial = 1.0molL−1

The rate initial is equal to 0.20 mol/L .

k = 0.2 sec.

[A] initial =  2.0 mol/L

[B] initial = 3.0 mol/L

Rate initials = 0.2 sec x 2.0 mol/L x 3.0 mol/L

rate initial = 2.4 sec.

Thus, the rate of the reaction is 2.4 mol/L x sec.

To learn more about rate of the reaction, refer to the below link:

https://brainly.com/question/13693578

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