For a hypothetical reaction:A + 2B + C>D +EThe rate law has been determined and is as follows:Rate = k[A][B]?What happens to the reaction rate when we make each of the following concentrationchanges?a) We triple the concentration of A without changing the concentration of B or C.b) We triple the concentration of B without changing the concentration of A or C.c) We triple the concentration of C without changing the concentration of A or B.d) We triple the concentrations of A, B and C simultaneously.e) We triple the concentration of D.

Ans: The rate of the given reaction can be expressed as follows: Rate = K[A][B]2 From the rate law…

Answered: For a hypothetical reaction: A + 2B +…

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...

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5. A certain reaction has a rate law of rate = k[C]. The activation energy for this reaction is 3.0000 x 104 J/mol, and the collision frequency is 2.000 x 10-³. If the desired reaction rate using an initial [C] of 0.0300 M is 1.00 x 10⁹ M/s, what must the reaction temperature be? You must first determine the value of the rate constant k, then use k, EA, and A to determine temperature. Show all work. 6 Find and cito lucing or
See attached image for question A.) What is the order of the reaction in A? B.) What is the rate of reaction when the initial concentrations are [A]= 0 M and [B]= 4.4x 10-2M?
Consider the following reaction: A+B+C →D The rate law for this reaction is as follows: Rate = k [A][C]² [B]¹/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.18x10-² M/s. Part A What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Rate 2 = Submit Provide Feedback IVE ΑΣΦ Request Answer ? M/s Review
A reaction was experimentally determined to follow the rate law, rate = k[X]2 where k = 0.860/M.s. If the starting concentration of X = 0.800 M, how many seconds will it take for the concentration of X to become 0.400 M? O (3) 0.465 sec O (4) 1.45 sec O (1) 0.805 sec O (2) 1.16 sec A Moving to the next question prevents changes to this answer. # T3 7 To D *3 E C 54 R F % 5 V T G 6 MacBook Pro B Y & N 7 H U N * 00 8 J 1 ( 9 K M O L P Question 12 of 37 > = است 11
Consider the reaction below at 100oC T2U (g) ⟶⟶ 2 T (g) + U (g) When [T2U] = 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U]o = 0.144 M, the reaction rate is 3.09 x 10-3 M/s, A. Which is the rate law of this reaction? B. which is the numerical value of the specific-rate constant, k, for this reaction? C. Which are the units for the specific rate constant, K? D. At whic rate is T generaten when [T2U] is 0. 111 M? E. if given an initial reactant concentration [T2U]o = 0.250 M, what is [T] after 15 minutes have elapsed?
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Which of the following statements about rate laws is FALSE? A) Rate laws can only be determined experimentally. B) Rate laws tell us information about the mechanism of the chemical reaction under study. C) The rate law for the chemical reaction A + B + 20 –D must be rate = k[A][B][C]² %3D D)A rate law can only be written for the elementary reactions of a given chemical reaction.
2.) The reaction below was found to have the rate law, rate = k[A][B] 2. For EACH of the scenarios below indicate by what factor the rate of reaction will increase: 2 A + B ↓ products a.) While holding the concentration of A constant, the concentration of B was increased from x to 3x. b.) While holding the concentration of B constant, the concentration of A was increased from x to 3x.c.) The concentrations of BOTH A and B were increased from x to 3x at the same time.
2
1. Given the following data, determine the orders (m and n) with respect to the concentrations of A and B in the reaction Orders: [A] 0.020 M 0.020 M 0.010 M 0.010 M m= A+B products Rate = k[A][B]" [B] 0.020 M 0.010 M 0.020 M 0.010 M n = Time for reaction 19 sec 19 sec 76 sec 76 sec What time would you predict if both concentrations of A and B were made to be 0.040 M?
The rate of a certain reaction is given by the following rate law: rate=k|N, || H2 K[N][H° Use this information to answer the questions below. What is the reaction order in N,? 1 х10 What is the reaction order in H2? ? 2 What is overall reaction order? 3 At a certain concentration of N, and H2, the initial rate of M reaction is 5.0 x 103 M / s. What would the initial rate of the reaction be if the concentration of N2 were halved? Round S your answer to 2 significant digits. The rate of the reaction is measured to be 0.640 M/ s when [N2] - 2 • S 1.8 M and [H2] 1.4 M. Calculate the value of the rate - 1 k = |M constant. Round your answer to 2 significant digits.

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