(c)According to Le Chatelier's principle, what conditions of (i) Temperature and (ii) pressurewould benefit the industrial preparation of Sulphur trioxide (SO3)2SO2(g) + O2SO3(g)AH =

Effect of Changing the Temperature According to Le Chatelier's Principle: To predict the direction…

Answered: (c) According to Le Chatelier's…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 38P

See similar textbooks

Similar questions

Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
Imagine that 3.60 mol of ammonia is placed in a 2.00 L vessel and allowed to decompose to theelements at 450oC:2 NH3 (g) 3 H2(g) + N2(g)If the experimental value of K is 6.3 for this reaction at 450oC, calculate the equilibriumconcentration of each reagent. What is the total pressure in the flask?
The Born-Haber process is, N2 (g) + 3 H2 (g) = 2 NH3 (g) has an equilibrium position when [N2] = 12.9 M, [H2] = 0.600 M and (NH3] =0.500 M. (a) What is the value of K? (b) If [N2] = 2.30 M, [H2] = 0.500 M and (NH3] =0.150 M, then are these concentrations at an equilibrium position? If not, then in which direction will a shift bring about equilibrium?
A 1.00-L flask was filled with 2.00 moles of gaseous SO2 and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, it was found that 1.34 moles of gaseous NO was present. Assume that the reaction SO-(9) + NO2 (g) = SO; (g) + NO(9) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. K =
Consider the reaction: 2 CO(g) + O2(g)=2 CO₂(g). The reaction is allowed to reach equilibrium in a sealed vessel. According to Le Chatelier's principle, what will happen to the equilibrium, if the volume of the vessel is decreased while the temperature is kept constant? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will be unchanged, but the reaction will shift to the right. (D) The equilibrium constant will increase and the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.
Exactly 1.0 mol N,04 is placed in an empty 1.O-L container and allowed to reach equilibrium described by the equation N204(s) = 2NO,(g). If at equilibrium the N,04 is 28.0% dissociated, what is the value of the equilibrium constant, K. for the reaction under these conditions? 0.44 O 2.3 0.31 0.78 0.11
A 1.00-L flask was filled with 2.14 mol gaseous SO2 and 2.14 mol gaseous NO2 and heated. After equilibrium was reached, it was found that 1.55 mol gaseous NO was present. Assume that the reaction SO2 (g) + NO, (g) = SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. HOW DO WE GET THERE? What are the equilibrium concentrations of SO2, NO2, and SO3? [SO2] = [NO2] = M [SO3] = M
When nitrogen and hydrogen are mixed in the ratio 1:3 at 50 atm and 650 °C, the equilibrium concentration of ammonia is 25% by weight. Calculate the equilibrium constant.
What pressure is required to achieve a CO2 concentration of 0.0690 mol L−1 at 20∘C?
Ammonia decomposes to form nitrogen and hydrogen, like this: 2 NH3(9)– N,(9)+3 H,(9) Write the pressure equilibrium constant expression for this reaction.
Bromine and water react to form hydrogen bromide and oxygen, like this: 2 Br,(g)+2 H,0(g)→4 HBr(g)+O2(g) Write the pressure equilibrium constant expression for this reaction.
Carbon monoxide and water vapor, each at 200. Torr, were introduced into a container of volume 0.250 L. When the mixture reached equilibrium at 700 degrees Celsius, the partial pressure of CO2(g) was 88 Torr. Calculate the value of K for the equilibrium CO (g) + H2O (g)⇋ CO2(g)+H2(g).

SEE MORE QUESTIONS

Recommended textbooks for you

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

(c) According to Le Chatelier's principle, what conditions of (i) Temperature and (ii) pressure would benefit the industrial preparation of Sulphur trioxide (SO3) 2SO2(g) + O2SO3(g) AH =