FOR PRACTICE 15.2 Consider the equation: CHCI3(8) + Cl2(8) CCI4(8) + HCI(g) The initial rate of reaction is measured at several different concentrations of the reactants with the tabulated results shown here. [CHCI3] (M) [Cl2] (M) Initial Rate (M/s) 0.010 0.010 0.0035 0.020 0.010 0.0069 0.020 0.020 0.0098 0.040 0.040 0.027 From the data, determine: (a) the rate law for the reaction (b) the rate constant (k) for the reaction

FOR PRACTICE 15.2 Consider the equation: CHCI3(8) + Cl2(8) CCI4(8) + HCI(g) The initial rate of reaction is measured at several different concentrations of the reactants with the tabulated results shown here. [CHCI3] (M) [Cl2] (M) Initial Rate (M/s) 0.010 0.010 0.0035 0.020 0.010 0.0069 0.020 0.020 0.0098 0.040 0.040 0.027 From the data, determine: (a) the rate law for the reaction (b) the rate constant (k) for the reaction

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

A certain reaction is first order in H, and first order in I,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [4.] [+] initial rate of reaction Calculator 圖 х10 0.429 M 0.563 M 0.0218 M/s olo 0.429 M 1.36 M |M/s 18 Ar I M/s 0.0981 M 2.46 M
One typical reaction occurring in car engines is NO2+ CO (g)--------> NO (g) + CO2 (g) In order to determine the order of the reaction and the rate constant k, a series of three experiments were performed. The results are shown in the table Experiment Initial [NO2] (mol/L) Initial [CO] (mol/L) initial rate (v) 0.0050 0.080 0.0050 0.10 0.40 0.10 0.10 0.10 0.20 1 2 3 1-Write down the general expression for the rate of this reaction 2- Find the order for each reactant and the overall order for this reaction. Show your work ( 3- Find the value for k. Show your work 4- Based on these data, do you think that this is an elementary step or not? Briefly explain (
1) Please help
3. Consider NO₂ (g) + CO (g) → NO (g) + CO₂ (g). The initial rates are shown in the table below. Please compute (a) the rate law for the reaction and (b) compute the value of k. [CO] 0.050 0.050 0.100 0.100 [NO₂] 0.050 0.100 0.200 0.100 Initial Rate (M/s) 0.0040 0.016 0.256 0.0640
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.
A reaction is identified as zero-order in one of its reactants, X. Time (s) [X] (M) 0 1.50 110 0.80 Based on the data and integrated rate law, what is the rate constant for the reaction at this temperature? k = [?] x 10 M-s-1 coefficient (green) exponent (yellow) Enter
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.
Question 17 of 23 Submit Butadiene reacts to form a dimer according to the equation 2C,H6(g) → C3H12(g) The reaction obeys the second order rate law, Rate = k[C,H,]?, with a rate constant k = 3.68 M-'min at a certain temperature. Starting with an initial concentration of [C,H] = 0.0500 M, what will be the butadiene concentration after 31.0 min? | M 1 2 3 C 7 9. +/- x 10 0 LO 00
Ln [A] Post Lab Assignment 1. Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl, (g) Determine the rate law, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) Rate (mol L-1 h-1) 0.10 0.20 0.30 3.2 x 10-9 7.2 x 10-9 2. A 5.0 mL dye solution of 3.45 e-5 M is mixed with 15.0 mL bleach solution of 0.21 M. What are the initial concentrations of [Dye] and [Bleach] for your experiment? 3. The plots of 1/[A] vs time, In([A]) vs. time, and [A] vs. time of a solution of substance A are shown below. What is the reaction order with respect to A? 000 009 007 000 0 20 40 Time (min) Time 09 08 Time
A + B +C → D Reaction [A] (М) [B] (М) [C] (М) Experiment Rate () 0.10 0.10 0.10 0.003 2 0.20 0.10 0.10 0.012 3 0.10 0.30 0.10 0.003 4 0.20 0.10 0.20 0.024 Determine the rate of the reaction when [A]= 0.30 M, [B] = 0.10 M and [C] = 0.20 M.