For the reaction 2 A + B + C, the initial rate is measured at several different reactant concentrations. From the resulting tabulated data, determine the rate law for the reaction. [A] (M) [B] (M) Initial Rate (M/s) 0.05 0.05 0.035 0.10 0.05 0.070 0.20 0.10 0.56 a) Rate = k[A][B] c) Rate = k[A][B]? b) Rate = k[A]²[B] d) Rate = k[A]°[B]²

For the reaction 2 A + B + C, the initial rate is measured at several different reactant concentrations. From the resulting tabulated data, determine the rate law for the reaction. [A] (M) [B] (M) Initial Rate (M/s) 0.05 0.05 0.035 0.10 0.05 0.070 0.20 0.10 0.56 a) Rate = k[A][B] c) Rate = k[A][B]? b) Rate = k[A]²[B] d) Rate = k[A]°[B]²

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 H2 (g) + 2 NO (g) + H,O (g) is studied at a certain temperature by determining the rate of reaction at reactant concentrations. The results are as follows: N,0 (g) 2. Concentration (M) Rate [NO] (i) (ii) [H] (M/s) 0.25 0.10 0.126 0.50 0.10 0.504 (iii) 0.50 0.20 1.03 The rate law is written as Rate = k [NO]* [H]°. The exponents x and y represent the order with respect to NO and H2, respectively. Calculate the value of x and y from the data provided.
For A⟶products, time and concentration data were collected and plotted as shown. [A] (M) t (s) 0.750 00.0 0.596 30.0 0.473 60.0 0.376 90.0 Determine the reaction order, the rate constant, and the units of the rate constant. order= k= units
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.
Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [N] [H] initial rate of reaction 0.335 M 2.47M 18.0M/s 0.335 M0.592M 1.03 M/s olo 0.521 M 2.47M 28.0 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|| Ix10 k = ||
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.
Initial rate data at a certain temperature is given in the table for the following reaction. [NOCI], (M) Initial rate of formation of Cl, (M/s) 2 NOCI(g) → 2 NO(g) + Cl, (g) 0.600 1.30 x 10-5 0.750 2.03 x 10-5 0.900 2.92 x 10-5 Determine the value and units of the rate constant, k. Units: k :
What is the rate constant without units?
Consider the reaction: A + B --> products. From the following data obtained at a certain temperature, determine the order of the reaction (rate law) and calculate the rate constant: [A] (M) [B] (M) Rate (M/s) 1.50 1.50 3.15 X 10-1 1.50 2.50 2.98 X 10 –1 3.00 1.50 5.50 X 10-1
or a reaction involving two reagents A and B, the following data was collected over three experiments. Exp# [A] [B] Rate (M/s) 1 0.20 M 0.20 M 5.0 2 0.20 M 0.40 M 20.0 3 0.10 M 0.40 M 10.0 Using the above data, which of the following is the rate law for the reaction of A with B?
The following kinetic data were obtained for the reaction A (g) + 2 B (g) → products Trial [A] (M) [B] (M) Initial Rate (M s-1) 1 0.60 0.30 0.0126 2 0.20 0.30 0.0014 3 0.60 0.10 0.0042 Determine the order with respect to A. Enter the answer as a single digit, not the word.
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]
Consider the following rate law: Rate = k[B] Which of the following equations could be used to find the concentration of B at some time (t) in the reaction? A) [B] = [B]₀ - kt B) [B] = [B]₀ × e^(-kt) C) 1/[B] = 1/[B]₀ + 2kt D) All of the above