For the reaction H 2 (g) + Br 2 (g) ⇌ 2HBr(g) , the relative amount of reactants and products present has to be described using the given K eq value. 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, aA+bB ⇔ cC+dD Forward reaction rate K f = [A] a [B] B Backward reaction rate K b = [C] c [D] d At equilibrium, the rate of forward reaction = rate of backward reaction K eq = K f K b K f K b = [C] c [D] d [A] a [B] B K eq = K f K b = [C] c [D] d [A] a [B] B K eq is the equilibrium constant.
For the reaction H 2 (g) + Br 2 (g) ⇌ 2HBr(g) , the relative amount of reactants and products present has to be described using the given K eq value. 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, aA+bB ⇔ cC+dD Forward reaction rate K f = [A] a [B] B Backward reaction rate K b = [C] c [D] d At equilibrium, the rate of forward reaction = rate of backward reaction K eq = K f K b K f K b = [C] c [D] d [A] a [B] B K eq = K f K b = [C] c [D] d [A] a [B] B K eq is the equilibrium constant.
Definition Definition Number that is expressed before molecules, ions, and atoms such that it balances out the number of components present on either section of the equation in a chemical reaction. Stoichiometric coefficients can be a fraction or a whole number and are useful in determining the mole ratio among the reactants and products. In any equalized chemical equation, the number of components on either side of the equation will be the same.
Chapter 9, Problem 9.77EP
(a)
Interpretation Introduction
Interpretation:
For the reaction H2(g) + Br2(g) ⇌ 2HBr(g), the relative amount of reactants and products present has to be described using the given Keq value.
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,
aA+bB⇔cC+dD
Forward reaction rateKf= [A]a[B]B
Backward reaction rate Kb= [C]c[D]d
At equilibrium, the rate of forward reaction = rate of backward reaction
Keq=KfKbKfKb=[C]c[D]d[A]a[B]B
Keq=KfKb=[C]c[D]d[A]a[B]B
Keq is the equilibrium constant.
(a)
Expert Solution
Explanation of Solution
The given reaction is:
H2(g) + Br2(g) ⇌ 2HBr(g)
Given,
Keq(25oC) = 2.0×109
The value of Keq is very large, so the products formed will be more than the reactants. Equilibrium will shift to the right.
Hence the product formed will be more.
(b)
Interpretation Introduction
Interpretation:
For the reaction 2HCl(g) ⇌ H2(g) + Cl2(g), the relative amount of reactants and products present has to be described using the given Keq value.
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,
aA+bB⇔cC+dD
Forward reaction rate Kf= [A]a[B]B
Backward reaction rate Kb= [C]c[D]d
At equilibrium, the rate of forward reaction = rate of backward reaction
Keq=KfKbKfKb=[C]c[D]d[A]a[B]B
Keq=KfKb=[C]c[D]d[A]a[B]B
Keq is the equilibrium constant.
(b)
Expert Solution
Explanation of Solution
The given reaction is:
2HCl(g) ⇌ H2(g) + Cl2(g)
Given,
Keq(25oC) = 3.2×10-34
The value of Keq is very small, so the reaction mixture will more of reactants. Equilibrium will be far to the left.
Hence the reactant will be more.
(c)
Interpretation Introduction
Interpretation:
For the reaction SO2(g) + NO2(g) ⇌ NO(g) + SO3(g), the relative amount of reactants and products present has to be described using the given Keq value.
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,
aA+bB⇔cC+dD
Forward reaction rate Kf= [A]a[B]B
Backward reaction rate Kb= [C]c[D]d
At equilibrium, the rate of forward reaction = rate of backward reaction
Keq=KfKbKfKb=[C]c[D]d[A]a[B]B
Keq=KfKb=[C]c[D]d[A]a[B]B
Keq is the equilibrium constant.
(c)
Expert Solution
Explanation of Solution
The given reaction is:
SO2(g) + NO2(g) ⇌ NO(g) + SO3(g)
Given,
Keq(460oC) = 85.0
The value of Keq is near to unity, so there are significant amounts of reactants and products in the reaction mixture.
(d)
Interpretation Introduction
Interpretation:
For the reaction COCl2(g) ⇌ CO(g) + Cl2(g), the relative amount of reactants and products present has to be described using the given Keq value.
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,
aA+bB⇔cC+dD
Forward reaction rate Kf= [A]a[B]B
Backward reaction rate Kb= [C]c[D]d
At equilibrium, the rate of forward reaction = rate of backward reaction
Keq=KfKbKfKb=[C]c[D]d[A]a[B]B
Keq=KfKb=[C]c[D]d[A]a[B]B
Keq is the equilibrium constant.
(d)
Expert Solution
Explanation of Solution
The given reaction is:
COCl2(g) ⇌ CO(g) + Cl2(g)
Given,
Keq(395oC) = 0.046
The value of Keq is near to unity, so there are significant amounts of reactants and products in the reaction mixture.
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The most common frequency in organic chemistry is the
Select one:
Oa. carbon-oxygen single bond
Ob. None of the above
Oc.
carbon-carbon double bond
Od. carbon-carbon single bond
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