Enter your answer in the provided box. Remember to enter your answer to the correct number of significant figures. For the reaction: A(g) + B(g) → AB(g) the rate is 0.25 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 = 3.1 mol/L and [B]0 = 3.5 mol/L?

8.409 mol/L.s

Explanation:

A(g) + B(g) → AB(g)

It is given that the reaction is first order in B and second order in A

R = k [A]² [B]

where R = rate of the reaction

k = rate constant

[A] = concentration of reactant A at any time

[B] = concentration of reactant B at any time

At the start of the reaction,

rate is 0.25 mol/L·s, when [A]₀ = [B]₀ = 1.0 mol/L

Substituting these into the rate equation, we solve for the rate constant

0.25 = k (1²) (1)

k = 0.25 L²/mol².s

The rate when [A]₀ = 3.1 mol/L and [B]₀ = 3.5 mol/L

R = 0.25 [A]² [B]

R = 0.25 × (3.1)² × (3.5)

R = 8.40875 = 8.409 mol/L.s

Hope this Helps!!

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