The liquid phase reaction A + 0.5B → C is first order in A and first order in B, and second order overall. Starting with an equimolar mixture, the reaction goes to 20% completion in 500 seconds. (Although CAo is not needed to solve the problem, for simplicity use CA0 = 1 mol/m³ for all parts) a. Is A or B the limiting reactant? b. Calculate the conversion of A and B. c. Plot the concentrations (CA/CA0 and CB/CA0, Cc/CA0) and rate of formation of C as a function of time. d. Plot the concentrations as a function of time if the reaction is first order in A and half order in B.

The liquid phase reaction A + 0.5B → C is first order in A and first order in B, and second order overall. Starting with an equimolar mixture, the reaction goes to 20% completion in 500 seconds. (Although CAo is not needed to solve the problem, for simplicity use CA0 = 1 mol/m³ for all parts) a. Is A or B the limiting reactant? b. Calculate the conversion of A and B. c. Plot the concentrations (CA/CA0 and CB/CA0, Cc/CA0) and rate of formation of C as a function of time. d. Plot the concentrations as a function of time if the reaction is first order in A and half order in B.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section14.6: Reaction Mechanisms

Problem 1RC: The rate equation for a reaction A + B C was determined by experiment to be Rate = k[A][B]. From...

See similar textbooks

Similar questions

One experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?
The gas phase reaction between hydrogen and iodine is proposed to occur as follows:.....step 1.....fast:......I2 2 I.....step 2.....slow:....H2 + 2 I 2 HI(1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism.Use the form k[A]m[B]n... , where '1' is understood (so don't write it if it's a '1') for m, n etc. Rate =
From the stoichiometry of the reaction 21(aq) + H2O2(aq) + 2H3O*(aq) → I2(s) + 4H2O(1) the rate law a. is predicted to be first-order in all reactants b. is predicted to be third-order overall c. is predicted to be first-order in I2(s d. cannot be predicted is predicted to be fifth-order overall е.
The following reaction was analyzed and data was collected. 3 A (g) + 2 B4 (g) + C2 (g) – D (g) Initial Concentration (mol L) (Ba] 0.100 Trial Initial Rate (mol Ls4) 9.072 x 109 3.629 x 10 2.449 X 107 3.135 х 10% [A] [C:] 1 0.100 0.400 2. 0.400 0.100 0.400 0.100 0.300 0.400 4 0.100 0.600 1.60 0.600 0.75 0.100 a) Determine the rate law and rate constant for the reaction. Be sure to show all of your work. b) Determine the rate for the fifth reaction.
For the rate law Rate = k[A][B]3/2, the order with respect to A is __________, the order with respect to B is __________, and the overall reaction order is __________.
1) a. b. If the rate of disappearance of O₂ is 0.125 M/s for a given time period, what is the rate of appearance of steam during this same time period? C. Write the rate expression for the reaction CsH12(g) + 802(g) → 5CO2(g) + 6H₂O(g).. d. What is the rate of reaction over this same time period? Verify this rate with at least two substances. Which substance in this equation reacts at the fastest rate? Which substance in this equation reacts at the slowest rate?
8. Consider the reaction: Trial # 1 2 3 4 5 6 2NH (g) + 302(g) + 2CH(g) → 2 HCN(g) + 6H₂O(g) [CH₂] (M) 0.37 0.45 0.45 0.26 0.45 0.17 [NH)] (M) 0.035 0.035 0.054 0.054 0.054 0.079 c. Write the rate law. b. Determine the overall reaction order. [0₂] (M) 0.12 0.27 0.12 0.27 a. Determine the order with respect to each of the reactants. 0.27 0.32 d. Solve for the value of the rate constant with units. Rate M/hr 2.3 x 10² 1.6 x 102 5.5 x 10² 3.7 x 102 3.7 x 10²
Br 1)what's the mechanism of the reaction? explain how does it work. fromeses Br Br 2)Give the correct stoichiometry/equivalence of the reaction (2 molecules per 1 molecule of what?) is there anything else that comes out of the reaction, if so what is it ■.
2. Here are representations of a reaction: A + B> products Unshaded spheres represent A molecules. Shaded spheres represent B molecules. Trial 1 Trial 2 Trial 3 Trial 4 Rate = 1 Rate = 1 Rate = 4 Rate = 4 a. What is the order with respect to A (unshaded)? Explain how you determined this. b. What is the order with respect to B (shaded)? Explain how you determined this. c. What is the rate equation for this reaction? Explain how you determined this.
Assessment Directions: Write the letter of the correct answer on your answer sheet. 1. Consider the rate law: rate - k[Y]=[Z]e. How are the exponents m and n determined? A. by experiment B. by educated guess C. by using the balanced chemical equation D. by using the coefficients of the chemical formula 2. For the reaction 2A + B+ 2C > D+ 2E, the rate law is: rate -k[A]F[B][C]!. Which of the following statements is false? A. the reaction is first order in [B] B. the reaction is 4th order overall C. the reaction is second order in (C] D. the reaction is second order in [A] 3. The reaction A + 2B – C is first order in B and A. The overall order of the reaction is A. first B. second C. third D. fourth 4. The reaction 2NO(g) + Ozlg) - 2NO:(g) has the following rate law: Rate - kļO2]|NO]2. If the concentration of NO is reduced by a factor of two, the rate will C. be reduced by one-half D. be reduced by one-quarter A. double B. quadruple 5. The rate of a reaction is found to double when the…
4. Hydrogen peroxide in basic solution oxidizes iodide ions to iodine. The proposed mechanism is H₂O₂(aq) + (aq) → HOI(aq) + OH(aq) slow HOI(aq) + (aq) → 12(aq) + OH(aq) fast a. Write the balanced reaction. b. Write a rate law consistent with this proposed mechanism. Rate =
Route 1:RME = 82.92%MI= 1.34 Route 2RME = 93.33%MI = 1.57 Route 3RME = 57.34%MI = 1.89 Compare the value of Reaction Mass Efficiency (RME) and Mass Intensity (MI) generally, and choose which metrics is more significant in green measurement. Justify your answer.