Show below in the table are the data from the decomposition of N2O5 in CCl4 at 45°C:Initial concentrationInitial rate, Ms-1of [N2O5], M0.50-41.55 × 103.10 × 10-44.65 × 104(a) Determine the order of the reaction (decomposition process).1.01.5(b) Calculate the value of k.(c) Then calculate the half-life of the above decomposition reaction.

First order kinetics means that the rate of the reaction depend on the concentration of the reactant…

Show below in the table are the data from the decomposition of N2O5 in CCI4 at 45°C Initial concentration Initial rate, Ms of [N2O5], M 1.55 × 10 3.10 × 10¬4 4.65 × 10* (a) Determine the order of the reaction (decomposition process). 0.50 1.0 1.5 (b) Calculate the value of k. (c) Then calculate the half-life of the above decomposition reaction.

Show below in the table are the data from the decomposition of N2O5 in CCI4 at 45°C Initial concentration Initial rate, Ms of [N2O5], M 1.55 × 10 3.10 × 10¬4 4.65 × 10* (a) Determine the order of the reaction (decomposition process). 0.50 1.0 1.5 (b) Calculate the value of k. (c) Then calculate the half-life of the above decomposition reaction.

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

In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g) →½ H2(g) + ½ I2(g) the following data were obtained: HI], M seconds 1.01 0.505 0.253 0.127 1.05x103 3.15x103 7.32x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.01 M is s and when the starting concentration is 0.505 M is S. (2) The average A(1/[HI]) / At from t= 0 s to t= 1.05x103 s is The average A(1/[HI]) / At from t= 1.05×103 s to t= 3.15×103 s is Ms!. (3) Based on these data, the rate constant for this order reaction is
??
The following data are for the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C. H2₂O₂(aq) > H₂O(l) + 12 O₂(g) [H₂O₂], M time, min 7.34x10-2 0 3.67x10-2 8.68 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is (2) Based on these data, the rate constant for this 1.84x10-2 9.20x10-3 17.4 min. 26.0 order reaction is min -1
146Pm decays via first-order kinetics (as do all radioactive isotopes) and has a half-life of 5.53 y.A sample initially contains 1.50% by mass 146Pm. a) How many years will it take for the 146Pm concentration to drop to 0.80 %?
(1) The oxidation of ammonia produces nitrogen and water via the following reaction: 4 NH3(g) +3 02(g) → 2 N2(g) +6 H₂O(1) If rate of formation of H2O(7) is 3.0 mol/(L. s) is, (a) What is the rate of formation of Nitrogen gas? (b) What is the rate of disappearance of Ammonia gas?
The half-life of a Phosphorous-32 (³2P), a radioactive isotope of phosphorous, is 14 days. If you start with 1.00 mole of 32P atoms, how many moles will you have left after 42 days? (A) 1.00 mol (B) 0.500 mol (C) 0.330 mol (D) 0.250 mol (E) 0.125 mol
17. If one defines the rate of the reaction 30 CH3OH +B10H14 0 10 B(OCH3)3 + 22 H2 as -A[B10 H14] At Rate = then the rate is also correctly expressed by 1 A[CH3 OH] At 1 ΔΒ(0CH> )s] At 1 A[H;] (a) Rate = 30 (b) Rate = 10 (c) Rate = 22 At (d) none of these. (e) all of these.
Complete the following table for the first order reaction: A → product [A] k (min1) Rate (mol/L min) 0.200 2.0 x 103 (c) (b) 0.0372 0.035 6.82 (a) 7.98 x 103 (a) (b) (c)
H2 reacts with ClF. Someone thinks this is the mechanism: H2(g) + ClF(g) → HCl(g) + HF(g) HCl(g) + ClF(g) → Cl2(g) + HF(g) (a) Write the balanced equation for the overall reaction. (b) Identify any intermediates in the mechanism, if any. (c) identify and catalysts in the mechanism, if any. (d) Write rate laws for each elementary reaction in the mechanism. (e) If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction?
Consider the second-order decomposition of A under the following conditions: The initial concentration of A is 0.161 M and after 117 s the concentration has decreased to 0.111 M. (a) What is the value of the rate constant k? 4.0 M-1*s-1 (b) What is the half-life of the reaction? 4.0
For a reaction that follows the general rate law, Rate = k[A]0[B]3, what will happen to the rate of reaction if theconcentration of A is tripled and the concentration of B is doubled?(a) Increase by a factor of 6(b) Increase by a factor of 8(c) Increase by a factor of 9(d) Increase by a factor of 12
The scenes depict four initial reaction mixtures for thereaction of A (blue) and B (yellow), with and without a solidpresent (gray cubes). The initial rate, -Δ[A]/Δt(in mol/L s),is shown for each sphere representing 0.010 mol and the con-tainer volume at 0.50 L.(a) What is the rate law in the absence of a catalyst?(b) What is the overall reaction order?(c) Find the rate constant.(d) Do the gray cubes have a catalytic effect? Explain.