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!!

the answer

explanation:

the capillary tube was too close to the bottom of the beaker.

the ruler may have moved.

water got into the capillary tube.

the temperature was not allowed to equilibrate in the 2-4 minutes.

i'm assuming that it's c.) red bank..