McQuarrie Rock GalloglyAttempt 3presented by Macmillan LearningConsider this initial rate data at a certain temperature in the table for the reactionOH(aq)Initial ratesOCI (aq) + (aq)OI (aq) + Cl(aq)Trial[OCI ]o(M)[I]o(M)[OH-]o(M)(M/s)10.001730.00173 0.5100.00030320.00173 0.003040.5100.00053430.00265 0.00173 0.6580.00036040.001730.00304 0.9490.000287Determine the rate law.Answer Bank[OCI]²[OCI]rate k[OH™][I-]Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books60°F4)10:31 PM5/30/2022O[OH-]²2[1-1² Answer Bankrate = k[OCI12[OC][OH][1]Determine the value of the rate constant for this reaction and the correct units.Unitsk =M-². s-1Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books10:31 PM"60°FO5/30/2022O[OH-]2Peup

The rate law for the reaction can be written as: rate=kOCl-xI-yOH-z ......(1) Here, x is the order…

Consider this initial rate data at a certain temperature in the table for the reaction OH(aq) [I]o [OH-]o OCI (aq) + (aq) OI (aq) + Cl(aq) Trial [OCI ]o (M) (M) (M) 1 0.00173 0.00173 0.510 2 0.00173 0.00304 0.510 3 0.00265 0.00173 0.658 4 0.00173 0.00304 0.949 Determine the rate law. rate = k [OH-]² (1-1² Answer Bank [OC] [OH™] [OCI] [1] Initial rates (M/s) 0.000303 0.000534 0.000360 0.000287

Consider this initial rate data at a certain temperature in the table for the reaction OH(aq) [I]o [OH-]o OCI (aq) + (aq) OI (aq) + Cl(aq) Trial [OCI ]o (M) (M) (M) 1 0.00173 0.00173 0.510 2 0.00173 0.00304 0.510 3 0.00265 0.00173 0.658 4 0.00173 0.00304 0.949 Determine the rate law. rate = k [OH-]² (1-1² Answer Bank [OC] [OH™] [OCI] [1] Initial rates (M/s) 0.000303 0.000534 0.000360 0.000287

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...

See similar textbooks

Similar questions

2A(g) + 3/2B(g) Experiment e b) D d) k= 12345 Initial rate (mol/L.s) →→ C(g) 0.25*10-4 2.25x10-4 0.50×10-4 1.00×10-4 0.75*10-4 Initial [A] (mol/L) 5x10-2 15x10-2 5x10-2 10×10-2 5x10-2 unit: Overall reaction order is Rate = K[A][B] Initial [B] (mol/L) Reaction order with respect to A is Reaction order with respect to B is 5x10-2 5x10-2 10x10-2 5x10-2 15x10-2 O " O Calculate rate constant (k) based on data from experiment 3:
[03mol/L Initial Rate mol/L.s S02 m 7/1ou 0.118 0.25 0.40 0.25 0.20 0.118 0.75 0.20 1.062 Q1 Consider the following reactions SO2+03 → SO3 +O2. A rate study of this reaction was conducted at 298 K. The data that were obtained are shown in the table (a) What is the order of reactions for S02 (b) What is the order of reactions for 03 (c) Write the rate law (d) Determine the value and units of the rate constant, k
Can my answers be checked please thank you .
4
In 2nd order reaction 2OH →→ H2O + O k = 1.47 x 1010 M-1 s-1. There is an initial OH concentration of [OH]0 = 1.88×10−4M. a)How long will it take for the OH concentration to decrease to 6.0997×10−5M?
Be sure to answer all parts. For the following general reaction, rate = k[A]2 and k=1.3 × 10 2 M¹g¹; A+B 2C Use this information to fill in the missing table entries. Experiment [A] (M) [B] (M) Initial rate (M/s) 1 0.013 0.250 2.20 × 10-6 2 0.026 0.250 3 0.500 2.20 × 10-6 1) Initial reaction rate in experiment 2: x 10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3: M
1.
What amount of time is required for the concentration of A to decrease from 0.800 M to 0.180 M in the zero- order reaction A->B? (k = 0.0567 M*s1)
Use this data to determine the value of the rate constant. Ex # [A] (M) [B] (M) Rate (M/hr) 1 .240 .120 2.00 2 .120 .120 .500 3 .240 .0600 1.00 Question 4 options: 289 per hour 579 per hour 8.3 per hour 0.0144 per hour 69.4 per hour .00346 per hour 0.060 per hour 0.0173 per hour 17 per hour 0.12 per hour
In 2nd order reaction 2OH →→ H2O + O k = 1.47 x 1010 M-1 s-1. There is an initial OH concentration of [OH]0 = 1.88×10−4M. a)How long will it take for the OH concentration to decrease to 6.0997×10−5M?
Rate = k [A] [B]² Overall reaction order would be A. 0 В. 1 С. 3 D. 2 What is the connection between rate and temperature ? A. There is no connection between the two B. Rate is indirectly connected to temperature C. Rate is directly related to temperature in exothermic reactions and indirectly related to temperature in endothermic reactions D. Rate is directly connected to temperature E. Rate is indirectly related to temperature in exothermic reactions and directly related to temperature in endothermic reactions