The KP for the reaction
is 2.05 at 648 K. A sample of SO2Cl2 is placed in a container and heated to 648 K while the total pressure is kept constant at 9.00 atm. Calculate the partial pressures of the gases at equilibrium.

Interpretation:
Partial pressures of the gases at equilibrium has to be calculated
Concept introduction:
Law of mass action: The rate of chemical reaction is directly proportional to the product of concentrations of reactant to products.
Multiple equilibria: If a reaction can be expressed as the sum of two or more reactions, the equilibrium constant for the overall reaction is given by the product of the equilibrium constants of the individual reactions.
The equilibrium constant for two separate equilibrium constants are,
For overall reaction, the equilibrium constant
Therefore,
Calculating equilibrium concentration:
- Express the equilibrium concentrations of all species in terms of the initial concentrations and a single unknown x, which represents the change in concentration.
- Write the equilibrium constant expression in terms of the equilibrium concentrations. Knowing the value of the equilibrium constant, solve for x.
- Having solved for x, calculate the equilibrium concentrations of all species.
Explanation of Solution
The given reaction is,
Given: Total pressure is
Construct ICE table as follows,
Initially, the pressure of
Again the change in pressure for
Solving quadratic equation as follows,
Out of the two values, the value of ‘x’ has to be less than the original concentration of reactants. So, the value of
At equilibrium,
Therefore, Partial pressures of the gases at equilibrium were calculated.
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Chapter 14 Solutions
CHEMISTRY 1111 LAB MANUAL >C<
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