Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine: 2NO (g) + Cl2(g) → 2NOCI(g) The following initial rates at a given temperature were obtained for the concentrations listed below. Experiment Initial Rate (mol-L-1.h-1) [NO]o (mol-L-1) [Cl2lo (mol·L-1) 1 2.21 0.25 0.25 19.89 0.75 0.25 3 6.63 0.25 0.75 Determine the order for each reactant. Determine the rate law and the value of k for the following reaction using the data provided. Answer:

Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine: 2NO (g) + Cl2(g) → 2NOCI(g) The following initial rates at a given temperature were obtained for the concentrations listed below. Experiment Initial Rate (mol-L-1.h-1) [NO]o (mol-L-1) [Cl2lo (mol·L-1) 1 2.21 0.25 0.25 19.89 0.75 0.25 3 6.63 0.25 0.75 Determine the order for each reactant. Determine the rate law and the value of k for the following reaction using the data provided. Answer:

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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The reaction of nitrogen dioxide and carbon monoxide in the gas state to form carbon dioxide and nitric oxide is represented by the equation: NO2(g)+CO(g)--->CO2(g)+NO(g) The following data were collected for the above reaction Experiment No [CO2] (M) [CO] (M) Initial Rate (M/s) 1 5.0*10-4 1.6*10-2 1.7*10-7 2 5.0*10-4 3.2*10-2 1.7*10-7 3 1.5*10-3 3.2*10-2 1.5*10-6 Determine the order of the reaction with respect to each reactant.
One typical reaction occurring in car engines is NO2+ CO (g)--------> NO (g) + CO2 (g) In order to determine the order of the reaction and the rate constant k, a series of three experiments were performed. The results are shown in the table Experiment Initial [NO2] (mol/L) Initial [CO] (mol/L) initial rate (v) 0.0050 0.080 0.0050 0.10 0.40 0.10 0.10 0.10 0.20 1 2 3 1-Write down the general expression for the rate of this reaction 2- Find the order for each reactant and the overall order for this reaction. Show your work ( 3- Find the value for k. Show your work 4- Based on these data, do you think that this is an elementary step or not? Briefly explain (
Hydrogen gas reduces NO to N2 in the following reaction: 2H, (g) + 2NO(g) 2H,0(g) + N, (g) The initial reaction rates of four mixtures of H, and NO were measured at 1500°C with the following results: Experiment [H2]o (M) [NO]o (M) Initial Rate (M/s) 0.212 0.136 0.0393 2 0.212 0.272 0.0789 0.424 0.544 0.624 0.848 0.544 2.50 4.
6. The oxidation of Br¯ by Br03 in acidic solution (H*) is described by the equation 5 Br (aq) + Br03 (aq) + 6 H* (aq) З Вrz (aq) + 3 H,0() Initial [Br ] (M) Initial [BrO3] (M) Initial [H*] (M) Initial Reaction Rate (M/s) 4.2 x 10-3 8.4 x 10-3 1.055 x 10-3 4.2 x 10-3 Experiment 1 0.404 0.250 0.100 2 0.808 0.250 0.100 3 0.404 0.125 0.250 0.100 4 0.404 0.050 (a) What is the reaction order with respect to each reactant? (b) Write the rate law. (e) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order
14. The data in the table below was collected for the following reaction at 425°C. 2 A(g) + 3 B(g) →3 C(g) +2 D(g) Trial 1 2 3 4 [A] i, M [B]i, M Initial Rate, M/s 0.100 0.050 1.0 × 10-3 0.050 0.050 2.5 × 10-4 0.100 0.100 2.0 × 10-3 0.150 0.100 4.5 x 10-3 a. What is the rate law for this reaction? b. What is the overall order of the reaction? 15. The rate constant for the following reaction is 3.00 x 10-3 M-1 min-1 at 500 K:
Reaction of nitrogen monoxide and hydrogen A student collects the data below for the reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) Trial [NO]i [H2]i Initial Rate (M/s) 1 0.050 M 0.050 M 0.0917 2 0.10 M 0.050 M 0.367 3 0.10 M 0.10 M 0.734 Write 2-3 sentences to describe how you determined the rate law for the reaction.
The data shows that the rate depends on the concentration of the reactants. How else can a chemist increase the rate of reaction?
10. The data below are for the reaction: 2 NO₂ (g) + F₂ (g) → 2 NO₂F (g) [NO₂] (M) 0.100 0.200 0.200 0.400 0.200 [F₂] (M) 0.100 0.100 0.200 0.400 0.400 Initial rate (M/s) 0.026 0.051 0.103 0.411 see part c a. Write the rate law for this reaction. b. Determine the rate constant for this reaction. Pay attention to units. c. Predict the initial rate of the reaction when [NO₂] = 0.200 M and [F₂] = 0.400 M. d. The mechanism of the reaction is suggested as two steps: NO₂+ F2 → NO₂F + F (fast) NO₂+ F→→ NO₂F (slow) Is your rate law consistent with this mechanism? Explain your answer, making any changes necessary to create consistency.
Consider the balanced chemical equation. H₂O₂ (aq) +31 (aq) + 2H+(aq) → I3¯¯(aq) + 2H₂O(1) In the first 11.0 s of the reaction, the concentration of I drops from 1.000 M to 0.752 M. Part A Predict the rate of change in the concentration of H₂O2 (A[H₂O2]/At). Express the rate to three significant figures and include the appropriate units. A[H₂O₂]/At = Submit Request Answer Part B Value μÀ HÅ Δ[13]/Δt = Value Predict the rate of change in the concentration of I3 (A[13¯]/At). Express the rate to three significant figures and include the appropriate units. Submit Request Answer Units Units ? www. ?
14. Consider the following reaction: 2 N₂O(g) → 2 N2(g) + O2(g) rate - k[N₂O] For an initial concentration of N₂O of 0.50 M, calculate the concentration of N₂O remaining after 2.0 min ifk -6.8 x 10³ s¹¹. A) B) 0.98 M 0.39 M C) 0.86 M D) 0.22 M E) 0.75 M
Consider this reaction: 2C1₂0, (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate = (1.31 M¹-8¹)[Chos S Suppose a vessel contains Cl₂O5 at a concentration of 0.690 M. Calculate the concentration of C1₂O5 in the vessel 3.50 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M ? CU x10 X S