For the reaction A+B+C -> D+E, the initial reaction rate was measured for variou

Question

For the reaction A+B+C -> D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected:

Trial [A] (M) [B[ (M) [C] (M) Initial rate (M/s)

1 0.20 0.20 0.20 6.0 x 10^-5

2 0.20 0.20 0.60 1.8 x 10^-4

3 0.40 0.20 0.20 2.4 x 10^-4

4 0.40 0.40 0.20 2.4 x 10^-4

Reaction order respect to A = 2

Reaction order in respect to B = 0

Reaction order in respect to C = 1

The value of the rate constant k for this reaction = 7.5*10^-3 M^-2 * s^-1

Given the data calculated in Parts A, B, C, and D, determine the initial rate for a reaction that starts with 0.75M  of reagent A and 0.90M  of reagents B and C?

Explanation / Answer

Given your data, the reaction law is:

Rate = k [a]^2 [c]

Therefore,

Rate = (7.5e-3) (.75M)^2 (.90M)

Rate = 0.00380 M/s

Related Questions

Navigate

• Browse (All)
• Browse F
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.