Antimony(V) chloride. SbCl5, decomposes on heating to give antimony(III) chloride, SbCl3, and chlorine.
A closed 3.50-L vessel initially contains 0.0125 mol SbCl5. What is the total pressure at 248°C when equilibrium is achieved? The value of Kc at 248°C is 2.50 × 10−2.
Interpretation:
The total pressure of the system at equilibrium has to be found.
Concept introduction:
Equilibrium constant
Consider the reaction where the reactant A is giving product B.
On rearranging,
Where,
Ideal gas equation is an equation that is describing the state of a imaginary ideal gas.
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
T is the temperature
Answer to Problem 14.138QP
The total pressure of the system at equilibrium is found to be
Explanation of Solution
Given,
The initial amount of
The volume of the vessel
The equilibrium constant
To find initial concentration of reactant
The initial concentrations of the
To find the equilibrium composition.
Using the table approach, the equilibrium concentrations of the reactants and the products can be found.
The equilibrium concentration values are then substituted into the equilibrium expression to get the change in concentration x.
On rearranging we get a quadratic equation.
On solving the quadratic equation the value of x obtained.
On solving we get two values for x, the logical value for x is taken.
Total concentration of the reaction mixture at equilibrium is the sum of the concentration of products and reactants.
To find the total pressure
At constant temperature,
Where
The total concentration is substituted in the ideal gas equation to get the total pressure.
The equilibrium composition of the given reaction mixture was found. The total concentration of the equilibrium mixture is then substituted in the ideal gas equation to get the value of total pressure.
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Chapter 14 Solutions
General Chemistry (Instructor's)
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