The equilibrium constant K p has to be found. Concept introduction: Equilibrium constant ( K c ) : A system is said to be in equilibrium when all the measurable properties of the system remains unchanged with the time. Equilibrium constant is the ratio of the rate constants of the forward and reverse reactions at a given temperature. In other words it is the ratio of the concentrations of the products to concentrations of the reactants. Each concentration term is raised to a power, which is same as the coefficients in the chemical reaction . Consider the reaction where the reactant A is giving product B. A ⇌ B Rate of forward reaction = Rate of reverse reaction k f [ A ] =k r [ B ] On rearranging, [ A ] [ B ] = k f k r = K c Where, k f is the rate constant of the forward reaction. k r is the rate constant of the reverse reaction. K c is the equilibrium constant. Equilibrium constant ( K c ) : A system is said to be in equilibrium when all the measurable properties of the system remains unchanged with the time. Equilibrium constant is the ratio of the rate constants of the forward and reverse reactions at a given temperature. In other words it is the ratio of the concentrations of the products to concentrations of the reactants. Each concentration term is raised to a power, which is same as the coefficients in the chemical reaction. Consider the reaction where the reactant A is giving product B. A ⇌ B Rate of forward reaction = Rate of reverse reaction k f [ A ] =k r [ B ] On rearranging, [ A ] [ B ] = k f k r = K c Where, k f is the rate constant of the forward reaction. k r is the rate constant of the reverse reaction. K c is the equilibrium constant. Equilibrium constant ( K p ) : For gaseous substances the concentration will be proportional to its partial pressure. The equilibrium constant for gaseous reactions can be expressed in terms of the partial pressures of the gaseous products and reactants, and it is called equilibrium constant K p . Ideal gas equation is an equation that is describing the state of a imaginary ideal gas. PV =n RT Where, P is the pressure of the gas V is the volume n is the number of moles of gas R is the universal gas constant (R=0 .0821LatmK -1 mol -1 ) T is the temperature
The equilibrium constant K p has to be found. Concept introduction: Equilibrium constant ( K c ) : A system is said to be in equilibrium when all the measurable properties of the system remains unchanged with the time. Equilibrium constant is the ratio of the rate constants of the forward and reverse reactions at a given temperature. In other words it is the ratio of the concentrations of the products to concentrations of the reactants. Each concentration term is raised to a power, which is same as the coefficients in the chemical reaction . Consider the reaction where the reactant A is giving product B. A ⇌ B Rate of forward reaction = Rate of reverse reaction k f [ A ] =k r [ B ] On rearranging, [ A ] [ B ] = k f k r = K c Where, k f is the rate constant of the forward reaction. k r is the rate constant of the reverse reaction. K c is the equilibrium constant. Equilibrium constant ( K c ) : A system is said to be in equilibrium when all the measurable properties of the system remains unchanged with the time. Equilibrium constant is the ratio of the rate constants of the forward and reverse reactions at a given temperature. In other words it is the ratio of the concentrations of the products to concentrations of the reactants. Each concentration term is raised to a power, which is same as the coefficients in the chemical reaction. Consider the reaction where the reactant A is giving product B. A ⇌ B Rate of forward reaction = Rate of reverse reaction k f [ A ] =k r [ B ] On rearranging, [ A ] [ B ] = k f k r = K c Where, k f is the rate constant of the forward reaction. k r is the rate constant of the reverse reaction. K c is the equilibrium constant. Equilibrium constant ( K p ) : For gaseous substances the concentration will be proportional to its partial pressure. The equilibrium constant for gaseous reactions can be expressed in terms of the partial pressures of the gaseous products and reactants, and it is called equilibrium constant K p . Ideal gas equation is an equation that is describing the state of a imaginary ideal gas. PV =n RT Where, P is the pressure of the gas V is the volume n is the number of moles of gas R is the universal gas constant (R=0 .0821LatmK -1 mol -1 ) T is the temperature
Solution Summary: The author explains the equilibrium constant, which is the ratio of the rate constants of forward and reverse reactions at a given temperature.
Definition Definition Study of the speed of chemical reactions and other factors that affect the rate of reaction. It also extends toward the mechanism involved in the reaction.
Chapter 14, Problem 14.127QP
Interpretation Introduction
Interpretation:
The equilibrium constant Kp has to be found.
Concept introduction:
Equilibrium constant(Kc): A system is said to be in equilibrium when all the measurable properties of the system remains unchanged with the time. Equilibrium constant is the ratio of the rate constants of the forward and reverse reactions at a given temperature. In other words it is the ratio of the concentrations of the products to concentrations of the reactants. Each concentration term is raised to a power, which is same as the coefficients in the chemical reaction.
Consider the reaction where the reactant A is giving product B.
A⇌B
Rate of forward reaction = Rate of reverse reactionkf[A]=kr[B]
On rearranging,
[A][B]=kfkr=Kc
Where,
kf is the rate constant of the forward reaction.
kr is the rate constant of the reverse reaction.
Kc is the equilibrium constant.
Equilibrium constant(Kc): A system is said to be in equilibrium when all the measurable properties of the system remains unchanged with the time. Equilibrium constant is the ratio of the rate constants of the forward and reverse reactions at a given temperature. In other words it is the ratio of the concentrations of the products to concentrations of the reactants. Each concentration term is raised to a power, which is same as the coefficients in the chemical reaction.
Consider the reaction where the reactant A is giving product B.
A⇌B
Rate of forward reaction = Rate of reverse reactionkf[A]=kr[B]
On rearranging,
[A][B]=kfkr=Kc
Where,
kf is the rate constant of the forward reaction.
kr is the rate constant of the reverse reaction.
Kc is the equilibrium constant.
Equilibrium constant(Kp): For gaseous substances the concentration will be proportional to its partial pressure. The equilibrium constant for gaseous reactions can be expressed in terms of the partial pressures of the gaseous products and reactants, and it is called equilibrium constant Kp.
Ideal gas equation is an equation that is describing the state of a imaginary ideal gas.
PV=n RT
Where,
P is the pressure of the gas
V is the volume
n is the number of moles of gas
R is the universal gas constant (R=0.0821LatmK-1mol-1)
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