A second-order-reaction of the type A +2 B→ P was carried out in asolution that was initially 0.075 mol dm3 in A and 0.030 mol dm3 in B. After1.0 h the concentration of A had fallen to 0.045 mol dm3. (a) Calculate therate constant. (b) What is the half-life of the reactants?The rate constant for the decomposition of a certain substance is1.70 x 10-2 dm³ mol-¹ s¹ at 24°C and 2.01 x 10-2 dm³ mol-¹ s¹ at 37°C.Evaluate the Arrhenius parameters of the reaction.A reaction 2 AP has a third-order rate law with k = 3.50 x 104 dmºmol2 s¹. Calculate the time required for the concentration of A to changefrom 0.077 mol dm3 to 0.021 mol dm³.

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A second-order-reaction of the type A +2 B→ P was carried out in a solution that was initially 0.075 mol dm3 in A and 0.030 mol dm in B. After 1.0 h the concentration of A had fallen to 0.045 mol dm3. (a) Calculate the rate constant. (b) What is the half-life of the reactants?

A second-order-reaction of the type A +2 B→ P was carried out in a solution that was initially 0.075 mol dm3 in A and 0.030 mol dm in B. After 1.0 h the concentration of A had fallen to 0.045 mol dm3. (a) Calculate the rate constant. (b) What is the half-life of the reactants?

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

A second-order-reaction of the type A +2 B→ P was carried out in a
solution that was initially 0.075 mol dm3 in A and 0.030 mol dm3 in B. After
1.0 h the concentration of A had fallen to 0.045 mol dm3. (a) Calculate the
rate constant. (b) What is the half-life of the reactants?
The rate constant for the decomposition of a certain substance is
1.70 x 10-2 dm³ mol-¹ s¹ at 24°C and 2.01 x 10-2 dm³ mol-¹ s¹ at 37°C.
Evaluate the Arrhenius parameters of the reaction.
A reaction 2 AP has a third-order rate law with k = 3.50 x 104 dmº
mol2 s¹. Calculate the time required for the concentration of A to change
from 0.077 mol dm3 to 0.021 mol dm³.

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