(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

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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).
Explain the effect of each of the following stresses on the position of the equilibrium SO;(g) 2 SO02(g) + 2 O2(g) The reaction as written is endothermic. (a) O2(g) is added to the equilibrium mixture without changing volume or temperature. (b) The mixture is compressed at constant temperature. (c) The equilibrium mixture is cooled. (d) An inert gas is pumped into the equilibrium mixture while the total gas pressure and the temperature are kept constant. (e) An inert gas is added to the equilibrium mixture with- out changing the volume.
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?
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.
The equilibrium constant for the reaction, 3 H2(g) + N2(g)= 2NH3(g), at a given temperature is 1.4 x 10–7. Calculate the equilibrium concentration of ammonia, if [H2] = 1.2 x 10–2 mol L–1 and [N2] = 3.2 x 10–3 mol L–1.
1.25 moles of NOClwere placed in a 2.50 L reaction chamber at 427ºC. After equilibrium was reached, 1.10 moles of NOCl remained. Calculate the equilibrium constant, Kc, for the reaction 2NOCl(g) -> 2NO(g) + Cl2(g).
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.
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.
Select the reaction for which K, = Kc. 2 CO, (g) + 2 CF,(g) =4 COF, (g) NH,NO, (s) = N,O(g) + 2H,O(g) 2 H, S(g) + SO, (g) = 3 S(s) + 2 H,O(g) O 2 Na, O, (s) + 2CO,(g) =2 Na,CO;(s) + 0,(g)
Phosphorus tribromide decomposes to form phosphorus and bromine, like this: 4 PBr,(9)→P(9)+6 Br,(g) Write the pressure equilibrium constant expression for this reaction. ?

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(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 =