The Contact process is used in the manufacture of sulphuric acid, H₂SO4. The equilibrium in the Contact process is shown below: 2SO2(g) + O2(g) 2SO3(g) AH-196 kJ mol-1 This is an example of important chemical industrial processes which exist as equilibrium systems. Discuss how kinetic and equilibrium factors are considered in order to decide appropriate reaction conditions for an industrial plant, using the Contact process as an example or any other appropriate example.

The Contact process is used in the manufacture of sulphuric acid, H₂SO4. The equilibrium in the Contact process is shown below: 2SO2(g) + O2(g) 2SO3(g) AH-196 kJ mol-1 This is an example of important chemical industrial processes which exist as equilibrium systems. Discuss how kinetic and equilibrium factors are considered in order to decide appropriate reaction conditions for an industrial plant, using the Contact process as an example or any other appropriate example.

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

There are 5 main factors that affect the equilibrium of a chemical system.
Given this equilibrium 2A(g)+3B———C(g)+4D+ energy Discuss what happens to this equilibrium if the temperature increases while the pressure is held constant. Make sure to include a discussion of rates of the forward and reverse reactions as well as changes in the concentrations of A, B, C and D.
Consider the reaction H2(g) + I2(g) → 2 HI(g). It is reported that an equilibrium mixture of this reaction system contains the following concentrations of the reacting species: Species Concentration (M) H2 1.18 x 10-2 I2 1.2 x 10-3 HI 2.59 x 10-2 Given this information, the equilibrium constant for this reaction may be calculated to have a value of:
A chemical engineer is studying the following reaction: HCH3CO2(aq)+CH3NH2(aq) → CH3CO2(aq) + CH3NH3(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.54. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound concentration expected change in concentration HCH,CO₂ 1.01 M O↑ increase CH3NH2 1.22 M O decrease O↑ increase O decrease O (no change) O (no change) A CH,CO, 0.64 M O↑ increase O decrease O (no change) CH, NH3 1.04 M O ↑ increase O decrease O (no change) HCH CO₂ 0.33 M O↑ increase O decrease O(no change) CHÍNH, 0.50 M O↑ increase O decrease O (no change) B CH,CO, 1.01 M O increase O decrease O (no…
The equilibrium constant, Kc, for the following reaction is 57.6 at 277 K. 2CH₂Cl₂ (g) CH4 (9) + CCl4 (9) When a sufficiently large sample of CH₂Cl₂ (g) is introduced into an evacuated vessel at 277 K, the equilibrium concentration of CC14 (g) is found to be 0.383 M. Calculate the concentration of CH₂Cl₂ in the equilibrium mixture. [CH₂Cl₂] = M
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g) C₂H₂(g) + 3H₂(g) K₂=2.x10-5 P He fills a reaction vessel at this temperature with 15. atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of C₂H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of C₂H₂ at right. Round your answer to 1 significant digit. yes no atm ☐ x10 X ?
Given the following reaction, the equilibrium constant, and the initial concentrations; answer the four bullet questions. 2 NO2 (g) - 2 NO (g) + O2 (g) Kc = 1.56 x 10-10 Initial Species Concentration (M) NO2 5.62 x 10-10 NO 3.99 x 10-16 O2 9.35 x 10-3 • Set up the equilibrium expression, and calculate the reaction quotient (Q). Note: ^ means "to the" Q = [ Select ] • How does Q compare to K? Q is [ Select]
Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)→2 HgO(5) At a certain temperature, a chemist finds that a 3.6 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 9.7 g O2 21.8 g HgO 10.2 g Calculate the value of the equilibrium constant K̟ for this reaction. Round your answer to 2 significant digits. K_ = 0
Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)→2 HgO(s) At a certain temperature, a chemist finds that a 7.0 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 7.0 g O2 5.8 g HgO 16.5 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = | x10
KINETICS AND EQUILIBRIUM Using an equilibrium constant to predict the direction of... A chemical engineer is studying the following reaction: 4 HC1(g) + O₂(g) → 2 H₂O(g) + 2Cl₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.31. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel A B с compound HC1 0₂ H₂O Cl₂ HCI 0₂ H₂O Cl₂ HCI 0₂ H₂O C1₂ pressure 5.09 atm 5.63 atm 3.31 atm 4.48 atm 3.91 atm 5.34 atm 3.90 atm 5.07 atm 2.74 atm 5.05 atm 4.48 atm 5.65 atm expected change in pressure O ↑ increase ↑ increase O ↑ increase O ↑ increase O ↑ increase ↑ increase ↑ increase O ↑ increase ↑ increase O ↑ increase ↑ increase ↑…
Are chemical reactions a "disturbance" of chemical equilibrium? Please explain why it is or why it is not.
Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(9)→2 HgO(s) At a certain temperature, a chemist finds that a 10. L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 12.7 g O2 13.4 g HgO 15.5 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = | Submit Assignm Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center| Access 43.203 FEB 19 MacBook Air