The reaction of nitrogen dioxide with fluorine 2NO2+ F2 → 2NO₂ F - is first order in NO2 and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n (don't enter 1) and concentrations taken to the zero power do not appear. Rate = S In an experiment to determine the rate law, the rate constant was determined to be 1.31 x 10-4 M¹s¹. Using this value for the rate constant, the rate of the reaction when [NO₂] = 4.92 M and [F2] = 4.59 M would be M/s.

The reaction of nitrogen dioxide with fluorine 2NO2+ F2 → 2NO₂ F - is first order in NO2 and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n (don't enter 1) and concentrations taken to the zero power do not appear. Rate = S In an experiment to determine the rate law, the rate constant was determined to be 1.31 x 10-4 M¹s¹. Using this value for the rate constant, the rate of the reaction when [NO₂] = 4.92 M and [F2] = 4.59 M would be M/s.

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 gas phase reaction of hydrogen with iodine H₂+I2 → 2HI is first order in H₂ and first order in I2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 2.03 x 10-18 M¹s¹. Using this value for the rate constant, the rate of the reaction when [H₂] = 0.0356 M and [1₂] = 0.0123 M would be M/s.
The gas phase reaction of hydrogen with iodine H₂+ 12 → 2HI is first order in H₂ and first order in I2. Complete the rate law for this reaction in the box below. Use the form [A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate In an experiment to determine the rate law, the rate constant was determined to be 2.39 x 10-18 M's. Using this value for the rate constant, the rate of the reaction when [H2]=0.0636 M and [12]=0.0154 M would be M/s. Submit Answer Retry Entire Group more group attempts remaining
3. An experiment was carried out to determine the rate law for the following reaction: 19152 2NO( )+0( ) → 2NO( ) Where the rate law is: par Rate = k[NO] [0] The experiment was repeated three times and the following data recorded: Experiment # Initial [NO] (M) Initial [0] (M) Rate (M/s) 1 ullo2 M0.015 0.015 2 0.030 0.015 3 0.015 0.030 of in Determine the value of x in the rate law (order of reaction with respect to NO) by comparing experiments 1 and 2 in Equation 13 reaction with respect to O₂) by comparing experiments 1 and 3 in equation 13. 0.048 0.192 0.096
Let’s consider the following reaction, X+2Y - Z After performing some experiments, let’s assume a researcher has determined the rate law for this reaction to be, Rate = k [X][Y]2 But later, a second researcher reports that the mechanism for this reaction is actually, 2Y- 1 (slow) X+1- Z (fast) In the previously determined rate law consistent with this mechanism? If not, why? What should be rate law predicted by this mechanism?
The reaction of nitrogen dioxide with fluorine 2NO2+F2-->2NO2F is first order in NO2 and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A]^m[B]^n, where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n .
The rate of a certain reaction is given by the following rate law: rate =k[N,][H,° Use this information to answer the questions below. What is the reaction order in N,? x10 What is the reaction order in H2? What is overall reaction order? Continue ©2022 McGraw Hill LLC. All Rights Reserved.
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Suggest a mechanism behind the reaction NO(g) + Cl2(g) à NOCl(g) + Cl(g) with the rate law rate = k [NO]2 [Cl2] This reaction cannot be a one step reaction because of its rate law. It is therefore a multistep reaction, where the slow step represents a reaction between 2 molecules of NO with one molecule of Cl2 (slow) 2NO + Cl2 à ………. (fast). à ………… NO + Cl2. à NOCl + Cl
The rearrangement of cyclopropane to propene at 500 °C(CH2)3CH3CH=CH2is first order in (CH2)3. During one experiment it was found that when the initial concentration of (CH2)3 was 0.170 M, the concentration of (CH2)3 dropped to 0.0491 M after 1304.0 s had passed.Based on this experiment, the rate constant for the reaction is ______s-1.
A scientist already determined the rate of the reaction is first order with respect to I - . Determine the rate law and the value of k for the following reaction using the data provided. Hint, you only need to find the reaction order for S2O82⁻ because it is first order for I - . After you find the reaction order for S2O82⁻ you need to calculate k. S2O82⁻ (aq) + 3 I⁻ (aq) → 2 SO42⁻ (g) + I3⁻ (aq) [S2O82⁻ ]i (M) [I⁻ ]i (M) Initial Rate (M -1 s -1 ) 0.30 0.42 4.54 0.44 0.42 6.65 Rate = 120 M-2s-1 [S2O82⁻]2[I⁻] Rate = 195 M-3s-1 [S2O82⁻]2[I⁻] Rate = 86 M-2s-1 [S2O82⁻][I⁻] Rate = 23 M-1/2s-1 [S2O82⁻][I⁻] Rate = 36 M-1s-1 [S2O82⁻][I⁻]
The reaction of IC1 with hydrogen 2IC1 + H₂ → I2 + 2HCl is first order in IC1 and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate =