The initial rates listed in the following table were determined for the reaction,2 NO (g) + Cl2 (g) 2 NOCI (g)ExperimentInitial [NO]120.130.2630.13Initial [Cl]Initial rate of consumption of Cl₂ (M/s)0.201.0 x 1020.204.0 x 1020.105.0 x 10What is the order of this reaction with respect to NO?What is the order of this reaction with respect to Cl₂?What is the overall order for the above reaction?What is the rate constant for the same reaction?

To determine the rate law the steps of calculation are given below.Write the general rate law form.…

Answered: The initial rates listed in the…

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 balanced equation for a given reaction is 4 X + 3 Y → P. The following data regarding initial reaction rates were collected in the lab. What is the rate law for the reaction? Trial [X] (M) [Y] (M) Rate (M/s) 1 0.020 0.060 3.40 x 10–3 2 0.020 0.120 2.72 x 10–2 3 0.080 0.060 1.36 x 10–2
Using the data in the table, calculate the rate constant of this reaction. k= A+B → C + D Trial [A] (M) [B] (M) 1 0.290 0.380 2 0.290 1.03 3 0.464 0.380 Units Rate (M/s) 0.0163 0.119 0.0261
A certain reaction is second order in N₂ and second order in H₂. Use this information to complete the table below. Round each of your answers to 3 significant digits. 0.460 M 0.460 M 1.43 M [¹2₂] 1.66 M 2.94 M 0.534 M initial rate of reaction 56.0 M/s M/S M/S 0 x10 X
Initial rates were measured for the following reaction and are listed in the table. A + 2B ⎯→ products Expt. Initial Concentrations Initial Rate (mol/L·s) [A] [B] 1 0.115 0.135 2.70 × 10−3 2 0.115 0.270 2.16 × 10−2 3 0.345 0.135 8.10 × 10−3 What is the order of the reaction with respect to A, with respect to B, and overall?
Consider the given reaction : 2HgC2(ag) + C204²(ag) – 2CH(ag) + 2CO2(g) + Hg2Cl2(s) Experiment [HgCl2] [C2O42] Initial rate 1 0.0836 M 0.202 M 5.2 x10-5 0.0836 M 0.404 M 2.08 x10-4 0.0418 M 0.404 M 1.04 x104 4 0.0627 M 0.606 M ? Calculate the initial rate for experiment 4. 3.50 x 10-4 M min-1 8.75 x 103 M min-1 1.20 x 10-4 M min-1 O 6.00 x 104 M min 1
The reaction 2 NO (g) + O2 (g) → 2 NO2 (g) occurs when automobile exhaust releases NO into the atmosphere. Use the following data to determine the order with respect to NO for this reaction. Trial [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.012 0.020 1.02 x 10-4 2 0.024 0.020 4.08 x 10-4 3 0.024 0.040 8.16 x 10-4 Enter the answer as a single digit, not the word.
Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2]and 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.
Some measurements of the initial rate of a certain reaction are given in the table below. [N-] |H2 initial rate of reaction 4 0.185 M 0.675 M 3.00 x 10“M/s 0.185 M 1.34M 1.18 x 10°M/s olo 0.236M 0.675M 3.83 × 10*M/s Ar 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 x10 k =
8. Given the initial rate data for the reaction A + B → C, determine the rate law for the reaction. [A] Initial Rate 1.31 x 104 5.24 × 104 1.31 x 104 [B] 0.0460 0.220 0.0920 0.220 0.0460 0.440
: Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.30 0.20 Rate (mol/L/h) 8.0 x 10-10 3.2 x 10-9 7.2 x 10-9
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.
Some measurements of the initial rate of a certain reaction are given in the table below. [N-] H2 initial rate of reaction 4 0.756M 0.169M 5.00 x 10*M/s 0.186M 0.169M 3.03 × 10°M/s olo 0.756M 0.0761 M 2.25 x 10*M/s Ar 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 [] Ox10 k = 0

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