Be sure to answer all parts. Re The following data were collected for the reaction between hydrogen and nitric oxide at 700°C: 2H2(g) + 2NO(g) → 2H2O(g) + N½(g) Experiment [H2] [NO] Initial rate (M/s) 1 0.010 0.025 2.4 x 10-6 2 0.0050 | 0.025 1.2 x 10-6 3 0.010 0.0125 0.6 x 10-6 (a) Determine the order of the reaction. Enter a number in the field below. 3 (b) Calculate the rate constant. Number: Units: Mls M1.s1 M² · s-1 • S M2. s

Be sure to answer all parts. Re The following data were collected for the reaction between hydrogen and nitric oxide at 700°C: 2H2(g) + 2NO(g) → 2H2O(g) + N½(g) Experiment [H2] [NO] Initial rate (M/s) 1 0.010 0.025 2.4 x 10-6 2 0.0050 | 0.025 1.2 x 10-6 3 0.010 0.0125 0.6 x 10-6 (a) Determine the order of the reaction. Enter a number in the field below. 3 (b) Calculate the rate constant. Number: Units: Mls M1.s1 M² · s-1 • S M2. 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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Consider the following data for the reaction: A + B → P Rate=k[A]m[B]n Experiment [A]o [B]o Initial Rate (M/s) 1 0.20 0.14 3.35 2 0.20 0.27 13.4 3 0.40 0.14 6.70 What is the numerical value for m and n? What is the rate constant k?
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Suppose you are studying the kinetics of the reaction between nitrogen monoxide and hydrogen gas. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 0.0050 0.0020 1.25 x 10–5 2 0.010 0.0020 5.00 x 10–5 3 0.0050 0.0040 2.50 x 10–5 Based on the data, choose the correct exponents to complete the rate law. rate=k[NO]x[H2]y x=? y=?
The reaction A + 2B → products has been found to have the rate law, rate = %3D k[A] [B]?. While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases. 27 0 9 6. 0 6
[item#2b] *refer to the photo below*
The data in the table below were obtained for the reaction: 2A+ 2B → 3C Experiment Number [A] (M) [В] (M) Initial Rate (M/s) 1 0.186 0.451 2.26 0.930 0.451 11.3 0.186 1.35 20.34 The rate law for this reaction is rate = O A. k[A]2 O B. k[A]²[B]2 O. k[A][B] O D. K[A][B]? O E. k[A]²[B]
The following data were collected for the reaction: 2A > 4B + C Time Concentration of A Concentration of B (minutes) (moles/L) (moles/L) 1.000 0.000 10 0.800 0.400 20 0.667 0.677 30 0.571 0.858 40 0.500 1.000 50 0.444 1.112 1. Make a graph of the concentrations of A and B versus time. Estimate the rate of disappearance of A and the rate of formation of B at t= 25 min and at t= 40 min. Compare the rates of disappearance of A and formation of B. What would you expect the rate of formation of C to be at t= 25 min and t=40 min? 2. Determine graphically whether the reaction in #1 above is a first order or a second order reaction. Calculate the rate constant for the reaction.
Subject- Chemistry
1) Please help
Write rate law for the chemical reaction ?
Experimental data for the reaction A + 2B → C have been plotted in the following three different ways. 0.05 -3.0 0.04 0.03 0.02 0.01 0 IvI 0 2 Time (s) 1/[A] 100 80 40 20 0 In[A] -3.5 -4.0 -4.5 -5.0 0 2 Time (s) 2 Time (s) What is the order of the reaction, and what was the initial concentration of A? O first-order, initial concentration = 10 M second-order, initial concentration = 10 M zero-order, initial concentration = 10 M O second-order, initial concentration = 0.1 M O first-order, initial concentration = 0.1 M
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T