The following initial rate data were obtained for 2 NO(g) + O₂(g) → 2 NO₂(g). [NO] [0₂]0 (-A[0₂]/At)o M-s¯1 0.0150 0.0100 0.0184 0.0300 0.0100 0.0738 0.0300 0.0300 0.2214 Experiment I II III What is the rate law for the reaction? (Example input format: 'rate = k. [A]^2. [B]¹.) What is the value of the rate constant at the temperature of the experiments? 4.0✓ What are the units of the rate constant? O M-¹5-1 O M-³5-1 O M-²5-2 O M-²5-1 chemPad XX → Help Greek

The following initial rate data were obtained for 2 NO(g) + O₂(g) → 2 NO₂(g). [NO] [0₂]0 (-A[0₂]/At)o M-s¯1 0.0150 0.0100 0.0184 0.0300 0.0100 0.0738 0.0300 0.0300 0.2214 Experiment I II III What is the rate law for the reaction? (Example input format: 'rate = k. [A]^2. [B]¹.) What is the value of the rate constant at the temperature of the experiments? 4.0✓ What are the units of the rate constant? O M-¹5-1 O M-³5-1 O M-²5-2 O M-²5-1 chemPad XX → Help Greek

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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A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [H, initial rate of reaction х10 1.26 M 0.560 M 76.0 M/s | M/s 1.26 M 0.272 M | M/s 5.70 M 0.124 M
Consider the following reaction: CaO(s) + CO₂(g) → CaCO3(s) The data found below are the results obtained from using different concentrations of each reactant to measure the initial rate of the reaction: Trial 1 2 3 4 [CaO] (mol L-¹) [CO₂] (mol L-¹) 0.0050 0.0150 0.0200 0.0150 0.0020 O 0.0021 mol L-1 O 0.0042 x 10-² mol L-¹ O 0.4167 mol L-1 O 0.0083 mol L-1 O 0.004 mol L-1 0.0020 0.0040 Determine the concentration of CO₂ during trial 3. Initial Rate (mol L-¹ s-¹) 1.50 × 10-3 0.0135 0.025 0.027
4
The following reaction was monitored as a function of time. 2H₂O₂ --> 2 H₂O + O₂ Time.(hr) [H₂O₂]. (M) 0 5.0 10.0 15.0 1.00 0.845 0.715 0.605 Which of the following statements is/are true? Multiple answers are possible. The general rate law for this reaction is rate = k[H₂O₂]². This reaction is first order in H₂O2. The rate constant is approximately 0.034. A plot of 1/[H2O2] versus time gives a straight line. This reaction is second order overall.
The reaction A → C was performed and the concentration vs. time data below collected. time, s 0 1 2 3 4 5 6 7 8 [A], mol/L 0.9541 0.5884 0.3629 0.2238 0.1380 0.08512 0.05250 0.03238 0.01997 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]x rate constant (without units) =
Q6. Answer the following questions based on the data provided: N203(g) - NO,(g) + NO,(g) Time (s) (N,O.] (M) 1.000 25 0.822 50 0.677 75 0.557 100 0.458 0.377 125 150 0.310 0.255 0.210 175 200 a. What is the overall order of the reaction? b. Calculate the value of the rate constant. c. What is the concentration of dinitrogen monoxide at 250s?
Consider the rate data at a certain temperature for the reaction 2NO(g) +2H2(g) →N2(g)+2H2O(g) Experiment [H₂] (M) 1 0.200 2 3 DHONOM 0.200 0.400 Determine the order of the reaction with respect to hydrogen... 1 2 [NO] (M) 0.200 3 0.400 0.400 Rate (M/s) 2.06x10-4 8.24x10-4 1.65×10-3
The reaction A →B is found to be first order. At 650 K, 45 % of A has been converted to B in 75.0 minutes. At 650 K, calculate the rate constant of this reaction with the unit s O A. 1.77 x 1045-1 O B. 3.59 x 102 s-1 O. 2.72 x 10-6 5-1 O D. 1.33 x 1045-1 E. 1.82 x 10-6 5-1
The following initial reaction rates have been measured for the following reaction NO2(g) + O3(g) -> NO3(g) + O2(g) Experiment: Initial Concentration (M) initial rate of the reaction O3 NO2 1 0.7 0.21 6.3 2 1.39 0.21 12.5 3 0.7 0.38 11.4 4 0.18 0.66 X a) Determine the order of and write the rate law of the reaction b) determine the value of K for the reaction. c) Find X
Consider the data shown here for the reaction NO2(g) + CO(g) -> NO(g) + CO2(g) The data shows the initial rate for the reaction for various concentrations of reagents. Expt L[NO2]t=0 [CO]t=0 initial rate (M/S) 0.0050 0.10 0.40 0.10 0.10 0.080 0.10 0.20 0.0050 What is the order of this reaction with respect to CO ? Oa. 2 Ob. 1 Oc. o 123
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.
[A] vs Time In[A] vs Time O 1/[A] vs Time Least Squares Plot The reaction A → C was performed and the concentration vs. time data below collected. time, s [A], mol/L 0.7983 0.1898 0.1077 0.07517 0.05774 0.04687 0.03944 0.03405 0.02995 [A] 0 reaction order = Check Submit Answer 1 Time, s 2 3 Try Another Version Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = K[A]* rate constant (without units) = Next> (1 of 1) Show Approach 2 item att 5 6 Hide Hint 7 8 A least squares line gives the best straight- line fit through any set of points but to get the right answer you need to figure out which plot gives the straight line.