Nitric acid is used in the starting material for the production of ammonium nitrate. Thefinal reaction in producing ammonium nitrate is:3HNO,(aq) – HNO,(aq) + H,O() + 2NO(9)Using your knowledge collision theory and the factors that affect the rate of a reaction,describe 3 ways that the rate of this reaction can be increased to produce moreammonium nitrate. Include specific reasons why it would increase. (A:3)

From the collision theory, If we increase concentration of reacting molecules more collision would…

Answered: Nitric acid is used in the starting…

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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REACTION ENGINEERING Consider a heterogeneous gas-phase catalytic reaction:AB(g)→A(g)+B(g) (Catalyst) The surface reaction mechanism follows three steps: AB(g) +S <----> AB*S (Adsorption)AB*S<----> B*S+A(g) (Surface reaction)B*S <---> B(g) + S (Desorption) (a) Derive the rate law assuming each of the three cases: (1) adsorption is rate-limiting, (2) surface reaction is rate limiting, and (3) desorption is rate-limiting. Express the overall reaction rate (- Tan) in terms of total number of sites on the surface, C. partial pressures of the gas species (ie., PA. PA and Pa), rate constants of adsorption, the surface reaction, and desorption (kaks, and ko), and the equilibrium constants of adsorption, the surface reaction, and desorption (ie., K. Ks and Ko). Hint: Based on the reaction mechanism, only AB and B are adsorbed on the surface, i.e., there is no evidence that A alone can be adsorbed on the surface.
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5. Consider the equation Cobaltic manganate + plumbous phosphite →Products a) Provide the balanced equation b) If one starts with 19.5g cobaltic manganate and 24.5g plumbous phosphite, calculate the masses of reactants and products assuming a 100% reaction
Choose all the statements that is correct A large negative free change for a reaction means that .... A) the reaction greatly favors formation of the products B) only a small amount of product is produced at equilibrium C) the equilibrium constant of the reaction is small D) the equilibrium constant of the reaction is large
REACTION ENGINEERING Consider a heterogeneous gas-phase catalytic reaction:AB(g)→A(g)+B(g) (Catalyst) The surface reaction mechanism follows three steps: AB(g) +S <----> AB*S (Adsorption)AB*S<----> B*S+A(g) (Surface reaction)B*S <---> B(g) + S (Desorption) (a) Derive the rate law assuming (1) surface reaction is rate limiting, and (2) desorption is rate-limiting. Express the overall reaction rate (- Tan) in terms of total number of sites on the surface, C. partial pressures of the gas species (ie., Pab Pa and Pb), rate constants of adsorption, the surface reaction, and desorption (ka,ks, and kd), and the equilibrium constants of adsorption, the surface reaction, and desorption (ie., Ka. Ks and Kd).
The cycle of copper reactions illustrates important principles of chemical reactions. The cycle begins with elemental copper, which in a first reaction is oxidized to copper(II) cation. Copper(II) is then carried through different solid forms. In the last step, copper(II) cation is reduced, the copper metal is regenerated, and the cycle is closed. The five key steps are 1. 3Cu(s) + 2NO, + 8H* → 3Cu²* (aq) + 4H2O+ 2NO 2. Cu (aq) + 20Н (аq) —> Сu(ОН),(s) 3. Cu(OH),(s) –→ CuO(s) + H2O 4. CuO(s) + 2H → Cu²* (aq) + H2O 5. Cu* (aq) + Zn(s) → Zn²*(aq) + Cu(s) 2+ 2+ 2+ cycle reactions. amount of reagents, present answers to the following questions. Assume that you wa carry out a sequence ord use the right Question 1 Question 2 Question 3 How many grams of zinc metal are needed to completely regenerate 1.19 g of copper in the fifth step in the cycle? By how much is zinc oxidized in the fifth reaction?
Given the following reaction and using the data in the table, determine the order of the reaction:2NO2(g)→2NO(g)+O2(g) Time (sec) [NO2 ] ln [NO2 ] 1/[NO2 ] 0 0.0100 -4.605 100 100 0.00648 -5.039 154 200 0.00479 -5.341 209 300 0.00380 -5.573 263 400 0.00315 -5.760 317 500 0.00269 -5.918 372 600 0.00235 -6.057 426 a. none of these b. second c. zero d. third e. first
Please try to solve in Extent Reaction or Molecular balance way. My professor wants to have the answer in that way not normal chemistry x y way. Thank you.
the sloution must be handwritten please... in details .. the unit must be in kgmol and follow the balanced equation
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Problem 3 Dibutyl phthalate (diester) is produced in a CSTR operated isothermally at 112°C. The rate of formation of the di-ester from phthalic anhydride and butanol being very fast, the controlling step, in the presence of sulphuric acid catalyst, is the conversion of mono-ester to the diester. The liquid phase reaction is: СЫН.(СООCН:)CООН + CН,ОН A C6H4(COOC4H6)2 + H2O D B The rate of the reaction is given by the expression -TA = kC; gmol/L.h where CA is the concentration of the mono-ester in gmol/L. The value of the apparent rate constant is given by: k = 0.7628 x 10ol1.965- L/gmol.h where T is the reaction temperature in K. The initial concentration of the mono-ester is 2.84 gmol/L and the density of the reaction mixture is 0.984 kg/L. (Molar mass of diester = 278) 1. In an existing plant consisting of a CSTR of 1.1 m diameter and 1.6 m height, the volumetric feed rate is 10 L/min. (a) Find the conversion achieved in an ideal CSTR. (b) If the conversion achieved in practice 68.5%…
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