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

Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0096 M's: 2 NH, (g) N, (g) +3 H, (e) Suppose a 2.0 L flask is charged under these conditions with 150, mmol of ammonia. How much is left 2.0 s later? You may assume no other reaction is Important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 8 D.P Consider this reaction: 250, ) - 2S0, (g)+0, (g) At a certain temperature it obeys this rate rate - (0.067 M)[so, Suppose a vessel contains SO, at a concentration of 0.28OM. Calculate how long it takes for the concentration of SO, to decrease to 0.025M. You may assume no other reaction is important. Round your answer to 2 significant digits. Djo X
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?
Using the above data, determine the order of the reaction with respect to A and B, and the rate law.
Please, provide everything with the physical state, and peovide the right answer
The recombination of l atoms in the gas phase in the presence of argon (which removes the energy released by the formation of an l-l bond, and so prevents the immediate dissociation of a newly formed l2 molecule) was investigated and the order of the reaction was determined by the method of initial rates. The initial rates of reaction of 2 l(g) + Ar(g) → l2(g) + Ar(g) were as follows: [l]0/( 10-5 mol dm-3) 1.0 2.0 4.0 6.0V0/(mol dm-3 S- 1) (a) 8.70 X 10-4 3.48 X 10-3 1.39 X 10-2 3. 13 X 10-2 (b) 4.35 x 10-3 1.74 x 10-2 6.96 x 10-2 1.57 x 10-1 (C) 8.69 X 10-3 3.47 X 10-2 1.38 X 10-1 3. 13 X 10-1The Ar concentrations are (a) 1.0 x 10-3 mol dm-3 , (b) 5.0 x 10-3 mol dm-3, and (c) 1.0 x 10-2 mol dm-3 . Find the orders of reaction w ith respect to I and Ar and the rate constant.
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?
The rate law for the reaction 2A → B is second order in A. The following figure represents samples with different concentrations of A; the red spheres represent molecules of A. In which sample will the reaction proceed most rapidly?
Which of the following is true for the rate law r= k[A]M[B]"? O A) The order of each species must be determined by experiment. B) Both m and n are restricted to positive integers. C) Both m and n can be obtained from the stoichiometry of the overall reaction. D) The overall order of the reaction is given by m x n.
The following reaction is observed to be second order with respect to NO and first order with respect to Br2. Br2 (g) + 2NO (g) --> 2NOBr (g)
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?