A first-order homogeneous reaction of A→ 3B is carried out in a constant pressure batch reactor. It is found that starting with pure A the volume after 12 min is increased by 70 percent at a pressure of 1.8 atm. If the same reaction is to be carried out in a constant volume reactor and the initial pressure is 1.8 atm, calculate the time required to bring the pressure to 2.5 atm. O 1 min 8 min O NOTG 3 min O 9 min

A first-order homogeneous reaction of A→ 3B is carried out in a constant pressure batch reactor. It is found that starting with pure A the volume after 12 min is increased by 70 percent at a pressure of 1.8 atm. If the same reaction is to be carried out in a constant volume reactor and the initial pressure is 1.8 atm, calculate the time required to bring the pressure to 2.5 atm. O 1 min 8 min O NOTG 3 min O 9 min

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

Question 7 For numbers 7 to 8: For the kinetics ABC, each step being first-order, for reaction occurring in a constant-volume batch reactor (only A present initially). Calculate k₁ tmax for each of the cases: K = K₂/k₁ = 10 1.00 0.30 0.25 NOTG O 0.42
The rate constant for the reaction of NaOH + CH3COOC2H5→ CH3COONa + C2H5OH is 182.7069 L/mol.min at 30oC and the initial concentrations of NaOH and CH3COOC2H5 are 0.1 M. The 2nd order liquid phase reaction was carried out in a continuously stirred tank type reactor by feeding an equal volume of sodium hydroxide and ethyl acetate at 30 oC, and the conversion rates obtained over time are given in the table below. According to this; Calculate the retention time for this reaction? t (min) 5 10 20 30 xA 0.9730 0.9748 0.9800 0.9829
2. Consider the kinetic data of the reaction of P + 2 Q + 2+ - PQ, + Z*and answer the succeeding questions: Experiment P (M) Q (M) Temp ("C) Initial Rate, M/s 1 0.01150 0.01200 0.00000 25 4.80 x 10-4 2 0.02300 0.01200 0.00000 25 1.92 x 10-3 3 0.01150 0.02400 0.00000 25 9.60 x 10-4 4 0.04600 0.01200 0.00000 25 7.68 x 10-3 5 0.01150 0.04800 0.00000 25 1.92 x 10-3 6 0.01150 0.01200 0.00000 10 5.10 x 10-5 0.01150 0.01200 0.00000 40 4.55 x 10-3 0.01150 0.01200 0.00500 10 4.98 x 10-5 0.01150 0.01200 0.01050 25 4.82 x 104 10 0.01150 0.01200 0.02100 40 4.44 x 10-3 A. Determine the rate order with respect to P. Determine the rate order with respect to Q. C. Determine the rate law of the reaction. What is the average rate constant? Indicate the appropriate units. E. What is the energy of activation and frequency factor of the reaction without the additive ion? Include the equation of the best fit line of the Arrhenius equation and RSQ Note: Use the calculated rate constant in set up 1 for 25°C…
5:30 PM Wed Mar 15 < ... Tap here or pull up for additional resources Question 24 of 75 What amount of time is required for the concentration of A to decrease from 0.800 M to 0.215 M in the zero-order reaction A → B? (k = 0.0567 M*s¯¹) 1 4 7 +/- 2 5 8 3 6 9 O S LTE 11% Submit x 100
Question 30 of 39 Submit The zero order reaction A → Products takes 63.5 minutes for the concentration of A to decrease from 0.970 M to 0.205 M. What is the value of k for this reaction? M/min 1 3 4 C 7 8 9 +/- х 100 Tap here or pull up for additional resources
A+B AB Trial [A] (M) [B] (M) Rate (M/s) 1. 0.200 0.200 2.00 x102 0.400 0.200 8.00x 10 3. 0.200 0.400 4.00 x 10 Vhat is the order for B in the reaction above? Edit Format Table e T?v a BIU A 12pt Paragraph v 2.
3:58 1 4 7 +/- Question 12 of 12 The zero order reaction A → Products takes 63.5 minutes for the concentration of A to decrease from 0.970 M to 0.283 M. What is the value of k for this reaction? 2 5 8 M/min 3 60 9 O Submit Tap here or pull up for additional resources XU x 100
Consider a pseudo-first order rate constant for the degradation of MTBE in a fully mixed batch reactor that is equal of k' = 0.054min - 1 What will be the half life of MTBE in the reactor in units of minutes (min)?- will a reaction time of 1 minute be sufficient to get 50% removal of the MTBE?
The rate constant for the second-order decomposition of ozone to oxygen is 18×10³ m'/mol/hr at 135 °C. What will be the conversion of ozone in a constant volume, isothermal batch reactor after 1 hour at 135 °C assuming an initial concentration of 103 mol/m?? At this time, what will be the rate of decomposition of the ozone? Repeat this analysis for a temperature of 145 °C, assume the reaction is irreversible and an activation energy of 55 kJ/mol.
Find the reaction order (n), reaction rate constant (k) and reaction rate general form using integral method. Integral method steps:1. Assume a first order reaction (n= 1) 2. Integrate the reaction rate to find CA and time linear relation 3. Plot CA versus time to see if you get a straight line. If not, the assumption is not correct andassume a second order reaction (n=2), and repeat same procedure till linear plot achieved I want full answer with all solution steps plz
The initial reaction rate for the elementary reactor 2A + В > 4C was measured as a function of temperature when the concentration of A was 2M and that B was 1.5 M -rA (mol/dm³.s) 0.002 0.046 0.72 8.33 Т (К) 300 320 340 360 a) Calculate the activation energy b) Calculate the frequency factor c) Calculate the rate constant as a function of temperature using T=300 Kas the base case
Fill in the table with the correct responses. Reaction Order Integrated Rate Law Linear Plot Rate constant (k) from the linear plot Half life (t1/2) zero [a] [b] [c] [d] first [e] [f] [g] [h] second [i] [j] [k] [l] Answer bank: 1/At = kt + 1/Ao ln A vs time negative of the slope (-m) log A vs time At = -kt + Ao At/k Ao/2k y-intercept A vs time slope (m) At = kt + Ao 1/A vs t lnAt = -kt + lnAo ln2/k 1/kAo