Water gas, a mixture of H2 and CO, is an industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon.b) What will happen to the concentration of of each reactant and product at equilibrium if more C is added?c) What will happen to the concentration of each reactant and product at equilibrium if H2O is removed? d) What will happen to the concentration of each reactant and product at equilibrium if CO is added?e) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased? (a) Write the expression for the equilibrium constant (K) for the reversible reactionAH = -90.2 kJ2H2(g) + CO(g) = CH3 OH(g)(b) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more H2 is added?(c) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CO is removed?(d) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CH3OH is added?(e) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if the temperature of the system is increased'(f) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more catalyst is added?41. Nitrogen and oxygen react at high temperatures.(a) Write the expression for the equilibrium constant (K.) for the reversible reactionN2(g) + O2(g) = 2NO(g)AH = 181 kJ(b) What will happen to the concentrations of N2, O2, and NO at equilibrium if more O2 is added?(c) What will happen to the concentrations of N2, O2, and NO at equilibrium if N2 is removed?(d) What will happen to the concentrations of N2, O2, and NO at equilibrium if NO is added?(e) What will happen to the concentrations of N2, O2, and NO at equilibrium if the volume of the reaction vessel is decreased?(f) What will happen to the concentrations of N2, 02, and NO at equilibrium if the temperature of the system is increased?(g) What will happen to the concentrations of N2, O2, and NO at equilibrium if a catalyst is added?42. Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke,essentially pure carbon.(a) Write the expression for the equilibrium constant for the reversible reactionC(s) + H2O(g) = CO(g) + H2(g)AH = 131.30 kJ(b) What will happen to the concentration of each reactant and product at equilibrium if more C is added?(c) What will happen to the concentration of each reactant and product at equilibrium if H20 is removed?(d) What will happen to the concentration of each reactant and product at equilibrium if CO is added?(e) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system isincreased?43. Pure iron metal can be produced by the reduction of iron(III) oxide with hydrogen gas.(a) Write the expression for the equilibrium constant (K) for the reversible reactionFe2O3(s) + 3H2(g) = 2Fe(s) + 3H2O(g)AH = 98.7 kJ(b) What will happen to the concentration of each reactant and product at equilibrium if more Fe is added?(c) What will happen to the concentration of each reactant and product at equilibrium if H20 is removed?(d) What will happen to the concentration of each reactant and product at equilibrium if H is added?(e) What will happen to the concentration of each reactant and product at equilibrium if the volume of the reaction vessel is

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Chemistry

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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

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Water gas, a mixture of H2 and CO, is an industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon. b) What will happen to the concentration of of each reactant and product at equilibrium if more C is added? c) What will happen to the concentration of each reactant and product at equilibrium if H2O is removed? d) What will happen to the concentration of each reactant and product at equilibrium if CO is added? e) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?

(a) Write the expression for the equilibrium constant (K) for the reversible reaction
AH = -90.2 kJ
2H2(g) + CO(g) = CH3 OH(g)
(b) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more H2 is added?
(c) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CO is removed?
(d) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CH3OH is added?
(e) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if the temperature of the system is increased'
(f) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more catalyst is added?
41. Nitrogen and oxygen react at high temperatures.
(a) Write the expression for the equilibrium constant (K.) for the reversible reaction
N2(g) + O2(g) = 2NO(g)
AH = 181 kJ
(b) What will happen to the concentrations of N2, O2, and NO at equilibrium if more O2 is added?
(c) What will happen to the concentrations of N2, O2, and NO at equilibrium if N2 is removed?
(d) What will happen to the concentrations of N2, O2, and NO at equilibrium if NO is added?
(e) What will happen to the concentrations of N2, O2, and NO at equilibrium if the volume of the reaction vessel is decreased?
(f) What will happen to the concentrations of N2, 02, and NO at equilibrium if the temperature of the system is increased?
(g) What will happen to the concentrations of N2, O2, and NO at equilibrium if a catalyst is added?
42. Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke,
essentially pure carbon.
(a) Write the expression for the equilibrium constant for the reversible reaction
C(s) + H2O(g) = CO(g) + H2(g)
AH = 131.30 kJ
(b) What will happen to the concentration of each reactant and product at equilibrium if more C is added?
(c) What will happen to the concentration of each reactant and product at equilibrium if H20 is removed?
(d) What will happen to the concentration of each reactant and product at equilibrium if CO is added?
(e) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is
increased?
43. Pure iron metal can be produced by the reduction of iron(III) oxide with hydrogen gas.
(a) Write the expression for the equilibrium constant (K) for the reversible reaction
Fe2O3(s) + 3H2(g) = 2Fe(s) + 3H2O(g)
AH = 98.7 kJ
(b) What will happen to the concentration of each reactant and product at equilibrium if more Fe is added?
(c) What will happen to the concentration of each reactant and product at equilibrium if H20 is removed?
(d) What will happen to the concentration of each reactant and product at equilibrium if H is added?
(e) What will happen to the concentration of each reactant and product at equilibrium if the volume of the reaction vessel is

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According to Le Chatelier's principle, if there's any change in the concentration, pressure or temperature of reactants or products, then it affects the equilibrium. But according to this principle, the equilibrium will adjust itself in such a way that it will balance out the change which is affecting the equilibrium.

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