3. The initial rate for the elementary reaction A + 2B 3C in a constant-volume batch reactorwas measured as a function of temperature when the concentration of A was 1 M and that ofB was 2.5 M and reported in the table below.-TA (mol/L/s)T (°C)0.00212250.007170.022535450.0657550.180650.466751.142.678595a. What is the activation energy?b. What is the frequency factor?C. Write the rate constant as a function of temperature using T = 300 K as the base case.

📍 Approach to solving the question: To solve for the activation energy (Ea), the frequency factor…

Answered: 3. The initial rate for the elementary…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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The formation of NO from Na and O is to be carried out in a small batch reactor. As a first approximation, we shall consider that the reaction time is more rapid than the time of cylinder compression, consequently, the reaction takes place isothermally in car eylinder at 2700 K, in a constant volume reactor (cylinder) and under a pressure of 20 atm, the initial concentration of N2 is 0.0696 mol/liter. By a specifying constant volume, we are assuming that reaction take place rapidly with respect to the movement of the piston in the cylinder. Consider that the feed consists of 77% N2, 15% Oz and 8% other gases, which may be considered inert. At this temperature the equilibrium constant (Ke-0.01). The reaction is reversible: Na + 0z + 2NO With a rate equation: Cho -TN, = k ( CN, Co, Ke Calculate: a) The equilibrium conversion of N2. b) The time required to achieve 80% of the equilibrium conversion. The formation reaction rate- constant k at this temperature is 1.11 liter mol.h' Hint: dx…
The decomposition of substance A was studied at constant temperature, the set of experimental data obtained was recorded in the following table. Is the reaction first or second order with respect to A?
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gas phase reactionA -> B + Ccarried out isothermally in a constant volume batch reactor of 100 L. An amount of 100 moles of pure A is initially placed in the reactor. The reactor is well mixed and the ideal gas equation holds. If the reaction is first order,-rA = kCA with k = 1 1/sCalculate the time required to consume 80% (moles) of A.
Q4) The reaction A + B = C + D proceeds to equilibrium at a temperature of 573 K. The mole fractions of the four reactive species satisfy the equilibrium relation. The feed to a reactor contains 2.0 mol of A, 3.0 mol of B, 0.5 mol of C and no mol of D. If K (573) = 5, Calculate: a) The mole fractions of the final product. b) The fractional conversion of the limiting reactant.
2.193 Toluene (C,H5CH3) is hydrogenated according to the two simultaneous chemical reactions C,H5CH3 + H2 C6H6 + CH4 (а) 2C,H5CH3 + H2 (C,H6)2 + 2CH4 (b) Initially, the reactor contains 40% toluene and 60% H2 (% mole). At the end of the operation, the reactor contains 10% toluene and 30% CH4 (% mole). Find: a. The mole fraction of the diphenyl, (C,H5)2, at the end of the operation b. The conversion of H2 c. Solve (a) and (b) when the following final composition is specified: The reactor contains 10% toluene and 40% H2 (% mole).
Decomposition of N2O5 in CC14 at 45°C is known to follow a First-order kinetics. The specific rate constant for this decomposition process at the above temperature is 6.32 × 10* s. (a) If the initial concentration of N2O5 was 0.500 M, then what will be the concentration of N2O5 remaining (not decomposed) after 2.00 hr? (b) For 90% of the N2O5 to decompose, how much time will be required? (c) From the following decomposition data of N2O5, calculate the activation energy (Ea). Ti = 35°C, k = 6.60 ×10-5 s and T2 = 65°C, k2 = 2.40 ×10 ³ s1.
Please help with a-f

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