W(g) + X(g) → Y(g) + Z(g) 1. (10-14 minutes) The following experimental data were obtained for the reaction represented above, Experiment 1 2 is 3 4 Initial [W] (mol L) 0.136 0.034 0.033 0.202 Initial [X (mol L) fate= 0.136 0.137 0.034 0.233 (a) Determine the order of the reaction with respect to reactant W. Justify your answer. Between 2 and 3 reaction rate multiplied by lo byt W stays Initial Reaction Rate (mol L s¹) 1.07 x 10² 1.08 x 10² 6.67 x 10 the Same so its (b) Determine the order of the reaction with respect to reactant X. Justify your answer. BeXuccis Second order because it gets multiplied by I but Feaction rate is 16. c) Write the rate law for the overall reaction. 2 K[x)²

W(g) + X(g) → Y(g) + Z(g) 1. (10-14 minutes) The following experimental data were obtained for the reaction represented above, Experiment 1 2 is 3 4 Initial [W] (mol L) 0.136 0.034 0.033 0.202 Initial [X (mol L) fate= 0.136 0.137 0.034 0.233 (a) Determine the order of the reaction with respect to reactant W. Justify your answer. Between 2 and 3 reaction rate multiplied by lo byt W stays Initial Reaction Rate (mol L s¹) 1.07 x 10² 1.08 x 10² 6.67 x 10 the Same so its (b) Determine the order of the reaction with respect to reactant X. Justify your answer. BeXuccis Second order because it gets multiplied by I but Feaction rate is 16. c) Write the rate law for the overall reaction. 2 K[x)²

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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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
Based on the details in the paragraph below, determine the order with respect to the "reactant". Explain your reasoning. You are working with a set of reactants and running an experiment. You've determined the concentrations of your reactants and have determined initial rates for these and specifically you are looking at one reactant. You've graphed the data for it in 3 ways: [A] vs t; In[A] vs t; and 1/[A] vs t. The r values for each graph are shown below. | [A] vs t In [A] vs t 1/[A] vs t 0.722 0.927 0.881
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?
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The reaction I (ag) + OCI (ag) → IO¯(aq) + Cl¯(ag) was studied, and the following data were obtained: [I], (mol/L) [OCI¯], (mol/L) Initial Rate (mol/L · s) 0.080 0.18 7.80 x 10- 0.040 0.18 3.90 × 10–2 0.020 0.090 9.80 x 10 -3 0.16 0.090 7.80 x 10–2 What is the rate law? (Use k for the rate constant.) Rate = Calculate the value of the rate constant. k = L/mol · s Calculate the initial rate for an experiment where both I and OCI are initially present at 0.16 mol/L. Rate = mol/L · •S
H₂O₂(aq) +31 (aq) + 2H*(aq) →→ 13¯(aq) + 2H₂O(l) If the concentration of I drops from 1.045 M to 0.760 M in 10.7 seconds, what is the rate of disappearance of H*? 7.99x10-2 MS1 1.78x10-2 MS-1 5.33x10-2 MS-1 2.66x10-2 MS1 4.00×10-² MS-1
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The rate of a certain reaction is given by the following rate law: rate =k N, O, Use this information to answer the questions below. olo What is the reaction order in N,? |x10 18 Ar What is the reaction order in 03? What is overall reaction order? At a certain concentration of N, and 03, the initial rate of reaction is 0.780 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 5.0 x 103M/s when [N2] = 1.1 M and [03] = 1.1 M. Calculate the value of - 3 -1 k = |M •S the rate constant. Round your answer to 2 significant digits.
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0092 M-s : 2 HI (g) - H, (g) +L, (g) Suppose a 450. mL flask is charged under these conditions with 150. mmol of hydrogen iodide. After how much time is there only 75.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. dlo x10 8. 미
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The following data were obtained for the reaction 2A → B: Time, min TA], mol/L 0.0962 0.0398 0.0156 10 20 40 60 80 0.0059 0.000428 0.000061 0.000009 (i) By plotting a suitable graph, determine the order of this reaction. (i) Calculate the rate constant of the reaction.
General Chemistry 4th Edition McQuarrie Rock Gallogly University Science Books presented by Macmillan Learning Initial-rate data at a certain temperature is given in the table for the reaction N,0,(g) → NO(g) + NO,(g) [N,03lo(M) Initial rate (M/s) 0.100 0.720 0.200 1.440 0.300 2.160 Determine the value and units of the rate constant. units: k = Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Scien MacBook Pro