7. A solution of A is mixed with an equal volume of a solution of B containing the same number of moles, and the reaction A+ B C occurs. At the end of 30 minutes, A is 50% reacted. How much of A will be left unreacted at the end of sixty minutes if the reaction is a. zeroth-order in both [A] and (B] b. first-order in [A] and zeroth-order in [B] c. first order in both [A] and [B]

7. A solution of A is mixed with an equal volume of a solution of B containing the same number of moles, and the reaction A+ B C occurs. At the end of 30 minutes, A is 50% reacted. How much of A will be left unreacted at the end of sixty minutes if the reaction is a. zeroth-order in both [A] and (B] b. first-order in [A] and zeroth-order in [B] c. first order in both [A] and [B]

Chemistry

10th Edition

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...

See similar textbooks

Similar questions

A reaction was shown to follow second-order kinetics. How much time is required for [A] to change from 0.500 M to 0.160 M? (k = 0.456 M⁻¹ s⁻¹)
A certain reaction, reaction A products, is first order with respect to A. Starting with [A] = 0.250M, it takes 45 min to reduce the concentration of A to 0.110M. What is its rate constant for this reaction? O 7.9 x 10-3 min 1 O 3.1 x 10-3 min 1 O 1.8 x 10-2 min 1 O 3.0 x 10-4 min' O 1.1 x 10-1 min 1
The reaction A + 2B C is zeroth in A and first-order in B. The rateof reaction is measured in M/s. a. If [B] halves, what happens to the rate? b. If A is consumed at 0.40 M/s, what is the rate at which C is produced?
What percentage of the initial amount of S02Cl2 2ilk remain after 2.25 hours?
The rate constant for a second-order reaction is 0.13 M1s1. If the initial concentration of reactant is 0.26 mol/L, it takes s for the concentration to decrease to 0.19 mol/L. O 5.3 O 0.18 O 11 O 1,4 O 0.017
Consider the hypothetical first-order reaction below: B D Which of the following statements is TRUE? I. Increasing the concentration of B by a factor of four will also increase the rate by the same magnitude. II. The concentration of B will decrease linearly over time. OI only ONeither I nor II Oll only Both I and II
The reaction below is second order in [A]: A- 2B + C A solution initially at 0.620 M in A is found to be 0.054 M after 48 min. What is the half-life for this reaction. O A. 13.6 O B. 2.9 Oc 4.6 OD. 14.4 OE. 5.3
Consider the first-order reaction shown below. The yellow spheres represent the reactant, A. The blue spheres represent the product, B. A B t=0 s t = 1.00 s
Many drugs decompose in blood by a first-order process. Two tablets of aspirin supply 0.60 g of the active compound. After 30 min, this compound reaches a maximum concentration of 2 mg/100 mL of blood. If the half-life for its breakdown is 90 min, what is its concentration (in mg/100 mL) 4.5 h after it reaches its maximum concentration?
The decomposition of a chemical follows the Zero order with a rate constant, k = 0.00543 M/s. If the initial concentration of the reactant is 2.32. what is the concentration after 900 seconds?. The decomposition of a chemical is in the second order with a rate constant, k = .0123 M-1min-1. If the initial concentration of the reactant is 0.765 M. What is the concentration after 15 minutes.
You have a second-order reaction for B which has an initial concentration of 30.00 moles in 15.00 L. If this process has a reaction constant k = 1.90x10-6 M-1s-1 What is the half-life of this reaction in second? In minutes? What is the concentration after the first half-life? What is the concentration after 5 half-lives? What is the concentration after 3.00x104 seconds? (hint: use the integrated rate equations!)
a) The reaction A(ag) → B(aq) is first-order with respect to A(aq). The concentration of A(aq) after 100.0 s of reaction is 0.555 M. The concentration of A(aq) after a further 400.0 s (500.0 s total) is 0.333 M. What will be the concentration of A(aq) after a further 500.0 s (1000.0 s total)? What is the half-life of the reaction? The temperature is 25.0 °C throughout the reaction. b) The reaction 2 A(aq) → B(aq) is second-order with respect to A(aq). When the concentration of A(ag) is 0.150 M and the temperature is 25.0 °C, the reaction rate is 0.1350 M/s. If we increase the concentration of A(aq) to 0.450 M and lower the temperature to 5.0 °C, the rate of reaction becomes 0.0300 M/s. What is the activation energy for this reaction?