Consider the following condition and find out the direction of the reaction (1) Q < K (2) Q > K (3) Q = K Concept introduction: Equilibrium is the condition at which the concentration of the reactant and the product are equal and the reaction can in move either forward means towards product formation or backward reaction means towards reactant formation. Equilibrium constant K c is defined as the ratio of the concentrations of the products raised to the power of their stoichiometric coefficients and reactants raised to the power of their stoichiometric coefficients. Reaction quotient Q is defined as the ratio at any point of the reaction of the concentration of the product raised to the power of their stoichiometric coefficients and reactant raised to the power of their stoichiometric coefficients. aA + bB→cC + dD K c = [ C ] c [ D ] d [ A ] a [ B ] b , equilibrium Q = [ C ] c [ D ] d [ A ] a [ B ] b To find: The direction of reaction shift at different value of the reaction quotient and the equilibrium constant.
Consider the following condition and find out the direction of the reaction (1) Q < K (2) Q > K (3) Q = K Concept introduction: Equilibrium is the condition at which the concentration of the reactant and the product are equal and the reaction can in move either forward means towards product formation or backward reaction means towards reactant formation. Equilibrium constant K c is defined as the ratio of the concentrations of the products raised to the power of their stoichiometric coefficients and reactants raised to the power of their stoichiometric coefficients. Reaction quotient Q is defined as the ratio at any point of the reaction of the concentration of the product raised to the power of their stoichiometric coefficients and reactant raised to the power of their stoichiometric coefficients. aA + bB→cC + dD K c = [ C ] c [ D ] d [ A ] a [ B ] b , equilibrium Q = [ C ] c [ D ] d [ A ] a [ B ] b To find: The direction of reaction shift at different value of the reaction quotient and the equilibrium constant.
Solution Summary: The author explains the direction of reaction shift at different values of the reaction quotient and the equilibrium constant.
Interpretation: Consider the following condition and find out the direction of the reaction
(1) Q < K
(2) Q > K
(3) Q = K
Concept introduction: Equilibrium is the condition at which the concentration of the reactant and the product are equal and the reaction can in move either forward means towards product formation or backward reaction means towards reactant formation.
Equilibrium constant Kc is defined as the ratio of the concentrations of the products raised to the power of their stoichiometric coefficients and reactants raised to the power of their stoichiometric coefficients.
Reaction quotient Q is defined as the ratio at any point of the reaction of the concentration of the product raised to the power of their stoichiometric coefficients and reactant raised to the power of their stoichiometric coefficients.
aA + bB→cC + dD
, equilibrium
To find: The direction of reaction shift at different value of the reaction quotient and the equilibrium constant.
Explain the fowlling.
(a) Metaalic K is dessloved in liquid NH3 to form dilute soloution. ...(i)
b).. more K is added to form conc.soloution.....(ii)
c).. soloution (i) & (ii) are evaporated completely.
d).. soloution (i) is treated with Fe2O3.
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