2) Consider the following reaction and associated rate law: X (g) + Y(g) → Z Rate = k[X] [Y] b Use the data in Table 1 in the following problems. Table 1 Reaction Data [X]。 (M) [Y]。 (M) Rate (M/s) 0.882 0.217 283. 07 0.882 0.451 624. 47 0.882 0.572 820.57 0.882 0.882 1308. 22 0.228 0.882 124.96 0.442 0.882 382. 56 0.67 0.882 804. 48 b) Use the Linear Regression method to estimate a, b, the reaction order k, and their standard deviations. In this approach, you analyze initial rate data by fixing the concentration of all but one species, say X. Next, the rate law equation is linearized through a logarithmic transformation and a least-squares analysis is used to obtain a and its standard devaition. The process is repeated by keeping (X) constant and varying [Y] to obtain b and its standard deviation. Finally, using a and b, the average value of k and its standard deviation are deduced. a +/- b = +/- || +/- Reaction order k +/-

2) Consider the following reaction and associated rate law: X (g) + Y(g) → Z Rate = k[X] [Y] b Use the data in Table 1 in the following problems. Table 1 Reaction Data [X]。 (M) [Y]。 (M) Rate (M/s) 0.882 0.217 283. 07 0.882 0.451 624. 47 0.882 0.572 820.57 0.882 0.882 1308. 22 0.228 0.882 124.96 0.442 0.882 382. 56 0.67 0.882 804. 48 b) Use the Linear Regression method to estimate a, b, the reaction order k, and their standard deviations. In this approach, you analyze initial rate data by fixing the concentration of all but one species, say X. Next, the rate law equation is linearized through a logarithmic transformation and a least-squares analysis is used to obtain a and its standard devaition. The process is repeated by keeping (X) constant and varying [Y] to obtain b and its standard deviation. Finally, using a and b, the average value of k and its standard deviation are deduced. a +/- b = +/- || +/- Reaction order k +/-

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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[References] The reaction I (ag) + OCI (aq) → IO¯(aq) + Cl¯(aq) was studied, and the following data were obtained: I], (mol/L) [OCI"], (mol/L) Initial Rate (mol/L · s) 0.12 0.16 7.80 x 10-2 0.060 0.16 3.90 x 10-2 0.030 0.080 9.80 x 10-3 0.24 0.080 7.80 x 10- What is the rate law? (Use k for the rate constant.) Rate Calculate the value of the rate constant. k = L/mol · s Calculate the initial rate for an experiment where both I and OcI are initially present at 0.16 mol/L. Rate = mol/L · s
Consider the reaction data. A⟶products ? (?) ? (?−1) 325 0.391 575 0.735 What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all values. x1= y1= x1= x2= Determine the rise, run, and slope of the line formed by these points. What is the activation energy of this reaction?
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Determine the rate law and the rate constant for this reaction. 13.125. The table contains reaction rate data for the reaction 2 NO(g) + Cl,(g)→ 2 NOCI(g) Initial Rate Experiment [NO], (M) [Cl_]o (M) (M/s) 1 0.20 0.10 0.63 0.20 О.30 5.70 0.80 0.10 2.58 0.40 0.20 Predict the initial rate of reaction in experiment 4. 13.126. An important reaction in the formation of photochemical smog is the reaction between ozone and NO: NO(g) + O3(g) → NO;(g) + O,(g) 2. 2. 3.
2 NO(g) + Br2 (g) → 2 NOB1(g) Initial Rate Experiment NO] (M) [Br2] (M) (mol/L's) 1 1.0 x 10-2 2.0 × 10-2 2.4 x 10-2 2 4.0 x 10-2 2.0 × 10-2 0.384 3 1.0 x 10-2 6.0 x 10-2 7.2 x 10-2 What is the order of the reaction with respect to [NO] and [Br2], and what is the overall order of the reaction? Order with respect to [NO] = Order with respect to [Br2] = Overall order
Which of the following reactions is impossible to occur as a single step? Cl2(g) --> 2 CI(g) OCI + H20(1) --> HOCI(aq) + OH NO(g) + Cl2(g) NOCI2(g) --> O 2 NO(g) + O2(g) 2 NO2(g) -->
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Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(g) → C(g) + 2 D(g) is
Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.273 0.763 2.83 0.273 1.526 2.83 0.819 0.763 25.47 What is the rate law for this reaction? Type the letter A. B. C. D, or E in this blank: A) Rate = k[A][B] B) Rate = k[A] C) Rate = k[A]*[B] D) Rate = k[A][B] E) Rate = k[P] What is the value of the rate constant for the above reaction? Type A, B, C, D, or E in the blank here: A) 38.0 B) 0.278 C) 13.2 D) 2.21 E) 42.0
H₂O₂(aq) +31 (aq) + 2H*(aq) →→ 13¯(aq) + 2H₂O(l) If the concentration of I drops from 1.045 M to 0.760 M in 10.7 seconds, what is the rate of disappearance of H*? 7.99x10-2 MS1 1.78x10-2 MS-1 5.33x10-2 MS-1 2.66x10-2 MS1 4.00×10-² MS-1
just need standard error for K
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