07 x05 x 10⁹ y ¹-1y`13 x 10¹¹ y ¹-13 x 10¹5 y-1 T (K) k (year-1)3231.17 x 10-83738.10 x 10-5423 6.93 x 10-²4731.42 x 1015231.06 x 10³5733.71 x 104determine the rate constant at 1000 KK 1₂ = ek IER

Answered: Image /qna-images/answer/46ef9058-984f-4d4c-ba26-6537f8dd4d4b.jpg

Answered: T (K) k (year-1) 323 1.17 x 10-8 373…

T (K) k (year-1) 323 1.17 x 10-8 373 8.10 x 10-5 423 6.93 x 10-2 473 1.42 x 101 523 1.06 x 103 573 3.71 x 104 determine the rate constant at 1000 K K 1₂ KI = e (1) E a R

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

At a given temperature, the elementary reaction A = B, in the forward direction, is first order in A with a rate constant of 0.0230 s-1. The reverse reaction is first order in B and the rate constant is 0.0590 s-1. What is the value of the equilibrium constant for the reaction A =B at this temperature? K = What is the value of the equilibrium constant for the reaction B =A at this temperature? K =
2. For the following reaction at 500 °C Cl2 (g) + H2 (g) 2 HCI (g) + the following data were collected: Experiment [H2 ] [ Cl2 ] Initial Reaction Rate 1 0.025 M 0.012 M 1.60 x 10 4 2 0.050 M 0.012 M 6.40 x 10 -4 3 0.050 M 0.048 M 6.40 x 10 -4 Give a rate law expression for this reaction and also calculate the value of the rate constant (k) for this reaction. What is the overall order of this reaction?
Determine the rate law and the value of k for the following reaction using the data provided. S20g2 (ag) + 31(ag) 2 SO42-(g) + 13 (a9) [S20g2-i (M) (M) Initial Rate (M/s) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33 Rate = [23 M-1/25-120g2-11/2 Rate = [120 M-251IS20g²-1²1] Rate = [195 M-351IS20g²-1²117? %3D Rate = [36 M-151IS208²-[] %D Rate = [86 M 2s-1S2082-1[2
Q1
Which statement does not accurately describe chemical equilbirum for a reversible chemical reaction A↔B? Assume the forward rate constant is k1 and the reverse rate constant is k-1, and assume both directions are first order). -d[A]/dt = d[B]/dt k1 = k-1 K = [B]eq/[A]eq K = k1/k-1 None of these
1
For the reaction A + B C + D, various initial rate measurements were run beginning with A and B only, and beginning with C and D only. From the data below, calculate the rate law for both the forward and backward reactions. Then determine the equilibrium constant for the reaction. Rate (M/s) 1.081 x 10 6.577 x 10 6.568 x 10 [A] 0.660 [B] 1.23 4.01 1.23 2.25 4.01 Rate (M/s) 7.805 x 10 1.290 x 10" 1.300 x 10 [C] 2.88 [D] 0.995 2.88 1.01 1.65 1.65
The rate constant for the reactionBr(g)+O3(g) --> BrO(g)+O2(g)was determined at the four temperatures shown in the table below. T (K) k [cm3/(molecule•s) 238 5.90 x 10-13 258 7.70 x 10-13 278 9.60 x 10-13 298 1.20 x 10-12 Plot the above data, and then use that data to calculate the activation energy for this reaction.
The reaction described by H, (g) + 1,(g) → 2 HI(g) has an experimentally determined rate law of rate = k [H2][I2] Some proposed mechanisms for this reaction are: Mechanism A (1) H, (g) + L,(g) 2 HI(g) (one-step reaction) Mechanism B (1) 1,(g) =2 1(g) (fast, equilibrium) k_1 (2) H, (g) + 2 I(g) –→ 2 HI(g) (slow) Mechanism C (1) I, (g) = 2 I(g) (fast, equilibrium) k_ k, (2) I(g) + H, (g) –→ HI(g)+H(g) (slow) (3) H(g)+I(g) → HI(g) (fast) Which of these mechanisms are consistent with the observed rate law? O mechanism A O mechanism B O mechanism C In 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficient to break the I-I bond in an I, molecule. Which mechanism or mechanisms are consistent with both the rate law and this additional observation? O mechanism B O mechanism C O mechanism A
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
Determine the rate law and the value of k for the following reaction using the data provided. NO,(9) + O3(g) – NO3(g) + O2(g) [NO,li (M) 0.1 0.1 [03li (M) Initial Rate (ms-1) 1 0.33 1.42 2 0.66 2.84 0.25 0.66 7.10 Rate = 43 M's INO,0,] S. -25c O Rate = 1360 M2s"INO,110,] S. Rate = 227 M25s INO,J[0,125 O Rate = 430 M?s INO,10,
2A(g) + 3/2B(g) Experiment e b) D d) k= 12345 Initial rate (mol/L.s) →→ C(g) 0.25*10-4 2.25x10-4 0.50×10-4 1.00×10-4 0.75*10-4 Initial [A] (mol/L) 5x10-2 15x10-2 5x10-2 10×10-2 5x10-2 unit: Overall reaction order is Rate = K[A][B] Initial [B] (mol/L) Reaction order with respect to A is Reaction order with respect to B is 5x10-2 5x10-2 10x10-2 5x10-2 15x10-2 O " O Calculate rate constant (k) based on data from experiment 3: