The following are initial rate data for: A+ B C Experiment Initial [A] Initial [B] Initial Rate 0.10 0.10 4.5 0.20 0.10 18.0 0.10 0.20 9.0 What is the rate law for the reaction? O Rate k[A]!B]? O Rate = k[A]°[B]² O Rate = k[A][B]° O Rate k(AB]- O Rate = k[A]'[B]? * Previous L. AS

The following are initial rate data for: A+ B C Experiment Initial [A] Initial [B] Initial Rate 0.10 0.10 4.5 0.20 0.10 18.0 0.10 0.20 9.0 What is the rate law for the reaction? O Rate k[A]!B]? O Rate = k[A]°[B]² O Rate = k[A][B]° O Rate k(AB]- O Rate = k[A]'[B]? * Previous L. AS

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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Calculate the rate constant considering the following rate data obtained at 25oC for the following reaction.
Some measurements of the initial rate of a certain reaction are given in the table below. [H] 12| initial rate of reaction 1.04M 2.34M 17.0M/s 1.04M 1.10М 7.99 M/s 0.109 M 2.34М 1.78 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k I| x10 0 k =
The following are initial rate data for: A + 2B - C + 2 D Experiment Initial [A] Initial [B] Initial Rate 1 0.10 0.10 0.300 0.20 0.10 0.600 3 0.10 0.20 1.200 What is the rate law? The rate law is Rate = k[A]?[B]1. The rate law is Rate = k[A]?[B]*. The rate law is Rate = k[A]?[B]°. The rate law is Rate = k[A]°[B]?. The rate law is Rate = k[A]²[B]².
For a reaction with the rate law below: Rate = k[A]? %3D a plot of In[A] vs. time gives a straight line. a plot of 1/[A] vs. time gives a straight line. a plot of 1/[A] vs. 1/time gives a straight line. O a plot of [A] vs. time gives a straight line. O a plot of log [A]o/[A] vs. 1/time gives a straight line. A Moving to another question will save this response. esc 20 F3 F1 F4 $4 1. 2. 4 Q W R. # 3
For the given equation at 800 °C: CO(g) + Ch(g) > COCh(g), the following data were collecica Experiment (COL(M) 0.96 1.92 0.96 (CH] (M) 1.60 1.60 3.20 Rate of appearance COCh (M/s) 0.121 0.242 0.484 Determine the Rate Law for the reaction From your Rate Law determined in question #1 above, determine the value of the rate constant WITH THE APPROPRIATE UNITS. ONLY If you could not answer #1 above, use this "mock" data to solve for k: Rate = K[ARB]?, with [A] = 1.00 M and B]o = 1.50 M, with a rate of 2.50 x 10-2 M/s.
4. Given: A +B O C Rate ( M sec ') 4.0X 10 -5 4.0 X 105 16 X 10-5 [] 0.1 [B] 0.1 0.1 0.2 0.2 0.1 Determine the rate law. Calculate the rate constant. Determine the rate when [A] = 0.05 and [B] = 0.10
Consider the reaction A + 2B = C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [A] [B] (M) (M) 0.20 0.010 4.8x10-4 2 0.20 0.020 9.6x10-4 3 0.40 0.010 1.9x10-3 Trial 1 Rate (M/s) What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B].
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What is the rate constant without units?
A + B +C → D Reaction [A] (М) [B] (М) [C] (М) Experiment Rate () 0.10 0.10 0.10 0.003 2 0.20 0.10 0.10 0.012 3 0.10 0.30 0.10 0.003 4 0.20 0.10 0.20 0.024 Determine the rate of the reaction when [A]= 0.30 M, [B] = 0.10 M and [C] = 0.20 M.
Given below is the data for the reaction. Calculate the value of the rate constant "k" with proper units. A + B → C Set [A] (M) [B] (M) Init, rate M-sec 1 0.050 0.200 5.0 x 10-5 2. 0.100 0.200 5.0 x 10-5 0.050 0.600 4.5 x 10-4 Determine the order in "A" Determine the order in "B" Substitute the order for A and B in the rate law equation below. Rate = k [A]' [B]