A reaction is performed to study the reaction of ICl with hydrogen:2 ICI+ H2→I2 + 2 HClThe following reaction rate data was obtained in four separate experiments.Experiment[ICI]o, M[H2]o, MInitial Rate, Ms13.18x10-36.35x10-310.1390.11320.2780.11330.1390.2251.26x10-240.2780.2252.52x10-2What is the rate law for the reaction and what is the numerical value of k?Complete the rate law in the box below.Remember that an exponent of 'l' is not shown and concentrations taken to the zero power do not appear.Rate =k =

A reaction is performed to study the reaction of ICI with hydrogen: 2 ICI + H2 I2 + 2 HC1 The following reaction rate data was obtained in four separate experiments. Experiment [ICI]o, M [H2]o, M Initial Rate, Ms-1 1 3.18×10-3 0.139 0.113 |6.35×10-3 1.26x10-2 2.52x10-2 2 0.278 0.113 3 0.139 0.225 4 0.278 0.225 What is the rate law for the reaction and what is the numerical value of k? Complete the rate law in the box below. Remember that an exponent of 'l' is not shown and concentrations taken to the zero power do not appear. Rate =

A reaction is performed to study the reaction of ICI with hydrogen: 2 ICI + H2 I2 + 2 HC1 The following reaction rate data was obtained in four separate experiments. Experiment [ICI]o, M [H2]o, M Initial Rate, Ms-1 1 3.18×10-3 0.139 0.113 |6.35×10-3 1.26x10-2 2.52x10-2 2 0.278 0.113 3 0.139 0.225 4 0.278 0.225 What is the rate law for the reaction and what is the numerical value of k? Complete the rate law in the box below. Remember that an exponent of 'l' is not shown and concentrations taken to the zero power do not appear. Rate =

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 reaction is performed to study the reaction of ICl with hydrogen: 2 ICI+ H, Iz + 2 HC1 The following reaction rate data was obtained in four separate experiments. Experiment [ICI]o, M [H]o, M Initial Rate, Ms-1 1 0.139 0.113 3.18x10-3 2 0.278 0.113 6.35x10-3 1.26x10-2 2.52x10-2 3 0.139 0.225 4 0.278 0.225 What is the rate law for the reaction and what is the numerical value of k? Complete the rate law in the box below. Remember that an exponent of 'l' is not shown and concentrations taken to the zero power do not appear. Rate = M2s1. k%3D
A chemistry graduate student is studying the rate of this reaction: 2NH₂(g) → N₂(g) + 3H₂(g) She fills a reaction vessel with NH, and measures its concentration as the reaction proceeds: time (milliseconds) 0 10. 20. [NH₂] 0.700M 0.331 M 0.157M 30. 0.0743 M 40. 0.0352M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate=& k= 0 X 님 S
A kinetics experiment was conducted based on the reaction: 2NO + H2 - N20 + H20 Use the following data from the experiment to determine the rate law for the reaction. Expt. # Initial rate 1.46 M/min INO]. [H:]0 1 0.021 0.065 2 0.021 0.260 1.46 M/min 3 0.042 0.065 5.84 M/min rate = k[NO] 2[H 2) 2 rate = k[NO] rate = k[NO] 2[H 2] rate = k[NO][H 2] rate = k[NO] 2
In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g) 2 NO2(g) + ½ O2(g) the concentration of N2O5 was followed as a function of time. It was found that a graph of In[N,05] versus time in seconds gave a straight line with a slope of -6.82x103 s and a y-intercept of -2.58 . Based on this plot, the reaction is first order in N205 and the half life for the reaction is seconds.
Consider the gaseous reaction of mononitrogen monooxide with molecular hydrogen to produce molecular nitrogen and water. What is the reaction rate between t = 10 s and t = 30 s? Time (s) [H2] 0 1.00 10 0.805 20 0.663 30 0.491 40 0.376 50 0.308 -0.0127 M/s 0.00785 M/s 0.0255 M/s 0.0157 M/s -0.0157 M/s
The following reaction was studied at a given temperature: CH3CI(g) + H20(g) → CH3OH(g) + HCI(g) From the rate data below, determine the reaction orders. Exp [CH3CI]o [H2O]o Initial Rate (M s1) 1 0.100 0.100 0.182 2 0.200 0.200 1.45 3 0.200 0.400 5.81 CH3CI: first order H2O: first order CH3CI: second order H,O: second order CH3CI: second order H,O: first order O CH3CI: first order H2O: second order
The reaction C2H5Cl(g) → C2H4(g)+ HCl(g) has a rate constant of approximately 3.10x10-5 s-1 at 600 K. What is the reaction rate (in M/s) if 115.5 g C2H5Cl is placed in an 8.00 L container at 600 K?
The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+NO₂ → N₂ + 2 H₂O Experiment [NH4+]o, M [NO₂ ]o, M Initial Rate, M. s-1 0.0358 1.45 x 10-6 0.0715 0.0358 0.0715 1 2 3 4 Rate = 0.128 0.128 0.255 0.255 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. k = 2.89 x 10-6 2.88 x 10-6 5.76 x 10-6 M-1.s-1
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The reaction A+B → C was investigated in a series of experiments with different initial concentrations of the two reactants. The following initial rates were observed. What is the overall reaction order? O 0 05 02 0 1 O 3 04 Experiment 1 Experiment 2 Experiment 3 Initial [A] 0.10 M 0.20 M 0.20 M Initial [B] 0.10 M 0.10 M 0.20 M Initial rate 1.60 x 10-2 mol L-1 s-1 3.20 x 10-2 mol L-1 5-1 3.20 x 10-2 mol L-1 5-1
A chemistry graduate student is studying the rate of this reaction: 2C1,O, (g) 2Cl₂ (g) +50₂ (g) She fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds: time (minutes) 0 10. 20. [C1,05] 40. 0.600M 0.172M 0.101 M 30. 0.0710M 0.0548M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X Ś
1. Given the following data, determine the orders (m and n) with respect to the concentrations of A and B in the reaction Orders: [A] 0.020 M 0.020 M 0.010 M 0.010 M m= A+B products Rate = k[A][B]" [B] 0.020 M 0.010 M 0.020 M 0.010 M n = Time for reaction 19 sec 19 sec 76 sec 76 sec What time would you predict if both concentrations of A and B were made to be 0.040 M?