(a)
Interpretation:
For the reaction
Concept Introduction:
Law of
The equilibrium constant is the product of molar concentrations of the product which is raised to its stoichiometric coefficients divided by the product of molar concentrations of the reactant which is raised to its stoichiometric coefficients.
Equilibrium Constant:
Consider a reaction,
Forward
Backward reaction rate
At equilibrium, the rate of forward reaction = rate of backward reaction
(a)
Explanation of Solution
The given reaction is:
Given,
The value of
Hence the product formed will be more.
(b)
Interpretation:
For the reaction
Concept Introduction:
Law of Chemical Equilibrium:
The equilibrium constant is the product of molar concentrations of the product which is raised to its stoichiometric coefficients divided by the product of molar concentrations of the reactant which is raised to its stoichiometric coefficients.
Equilibrium Constant:
Consider a reaction,
Forward reaction rate
Backward reaction rate
At equilibrium, the rate of forward reaction = rate of backward reaction
(b)
Explanation of Solution
The given reaction is:
Given,
The value of
Hence the reactant will be more.
(c)
Interpretation:
For the reaction
Concept Introduction:
Law of Chemical Equilibrium:
The equilibrium constant is the product of molar concentrations of the product which is raised to its stoichiometric coefficients divided by the product of molar concentrations of the reactant which is raised to its stoichiometric coefficients.
Equilibrium Constant:
Consider a reaction,
Forward reaction rate
Backward reaction rate
At equilibrium, the rate of forward reaction = rate of backward reaction
(c)
Explanation of Solution
The given reaction is:
Given,
The value of
(d)
Interpretation:
For the reaction
Concept Introduction:
Law of Chemical Equilibrium:
The equilibrium constant is the product of molar concentrations of the product which is raised to its stoichiometric coefficients divided by the product of molar concentrations of the reactant which is raised to its stoichiometric coefficients.
Equilibrium Constant:
Consider a reaction,
Forward reaction rate
Backward reaction rate
At equilibrium, the rate of forward reaction = rate of backward reaction
(d)
Explanation of Solution
The given reaction is:
Given,
The value of
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Chapter 9 Solutions
CHM 104/201 <C>
- Based on the diagrams, chemical reaction, and reaction conditions depicted in Problem 9-81, for which of the diagrams is the numerical value of the equilibrium constant the smallest?arrow_forwardBased on the diagrams, chemical reaction, and reaction conditions depicted in Problem 9-83, which of the diagrams represents the equilibrium mixture if the numerical value of the equilibrium constant is 9.0?arrow_forwardConsider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the amount of ammonia at equilibrium be affected by 1. removing O2(g)? 2. adding N2(g)? 3. adding water? 4. expanding the container at constant pressure? 5. increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forward
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- What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.arrow_forwardWrite an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a productarrow_forwardThe value of the equilibrium constant, K, is dependent on which of the following? (There may be more than one answer.) a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.arrow_forward
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