The reaction X->Y follows first order kinetics. Initially a different number of X molecules is placed in three containers of equal volume at the same temperature as diagrammed below: A в a) If the rate of the reaction in container A is RA, express the initial rate of the reaction in containers B and C in terms of Ra. b) If the half-life of the reaction in container A is x (i.e. t/2 = x), give the half-life of the reaction in containers B and C in terms of x. c) If the volume of each container is doubled, the initial rates of the three reactions are R'a, R'B, and R'c. Express each of the R' initial rates in terms of Rạ. Container A Container B Container C а) RA RB Rc = b) t1/2 = x t1/2 = t1/2 = c) R'A = R'g = R'c =

The reaction X->Y follows first order kinetics. Initially a different number of X molecules is placed in three containers of equal volume at the same temperature as diagrammed below: A в a) If the rate of the reaction in container A is RA, express the initial rate of the reaction in containers B and C in terms of Ra. b) If the half-life of the reaction in container A is x (i.e. t/2 = x), give the half-life of the reaction in containers B and C in terms of x. c) If the volume of each container is doubled, the initial rates of the three reactions are R'a, R'B, and R'c. Express each of the R' initial rates in terms of Rạ. Container A Container B Container C а) RA RB Rc = b) t1/2 = x t1/2 = t1/2 = c) R'A = R'g = R'c =

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

The reaction A → B + C is zero order with respect to A. When [A]0 = 0.858 M, the reaction is 23.4 % complete at 96.7 min. Calculate the half-life for this reaction.
She fills a reaction vessel with H2CO3 and measures its concentration as the reaction proceeds. Here's a graph of her data: (W) [200³H] 2 1.5- 0.5 0 0 t(s) Use this graph to answer the following questions: What is the half life of the reaction? Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in 11/2 = ☐ s S ☐ x10 H2CO3. Calculate the value of the rate constant k. k = ☐ Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of H2CO3 in the engineer's reaction vessel after 5.0 seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in H2CO3. Round your answer to 2 significant digits. [H₂CO,] = M
For the reaction A → B, a plot of ln[A] vs. time yields a straight line with the equation y= -0.423 + 0.092x. What is the reaction order with respect to A? What is the half-life of the reaction in (s) ? What was the initial concentration of A (M) ?
The rate equation for a reaction: A → B is r=K[A]0 . If the initial concentration of the reactant is a moldm-3 , the half-life period of the reaction is?
The reaction N2O5- 2NO2 + 1/2 O2(g) is first order. The rate constant k is 6.2 x 10-4/min. A) What is the half life of this reaction in seconds and days? B) How long will it take for the concentration of N2O5 to decrease to 25% of it's original concentration?
The reaction A(aq) ---> B(aq) + C(aq) is a first order reaction. The half-life of A(aq) is 93.4 s at 25.0oC and its half-life is 71.7 s at 45.0oC. What is its half-life (in s) at 65.0oC?
a) What are the units of the rate constant for a zero-order reaction?b) What are the units of the rate constant if rate =k[A]5[B]3[C]?c) What is the order of reaction for part (b) of this question?
The reaction A + 2B → products was found to be first-order to A and second- order to B. Predict by what factor will the rate of reaction increase when the concentration of A and B are increased to 2 times of the original values at the same time? Please report an integer, without units.
The reaction A+2B ——> products was found to be first order to A and second order to B. While holding the concentration of A constant , the concentration of B is increased to 3 times its initial value . By what factor does the rate of reaction increase?
Be sure to answer all parts. The reaction 2A →B is second order with a rate constant of 51.0/M· min at 24°C. (a) Starting with [A]0 = 8.90 ×10−3 M, how long will it take for [A]t = 3.40 ×10−3 M? (b) Calculate the half-life of the reaction.
The reaction A(aq) ---> B(aq) is a first order reaction with respect to A(aq). The concentration of A(aq) is reduced to 35.0% of its initial value in 1.49 minutes. What is the value of the half-life (in s) of the reaction?
The half-life of a radioactive plutonium-246 was found to be 215 years. If its initial concentration is 6.4 M and follows the first-order reaction, how long will it take to reach a concentration of 0.5 M? [Stoichiometric coefficient for the reactant, a=1].