# Problem: At 25ºC, gaseous SO2Cl2 decomposes to SO2(g) and Cl2(g) to the extent that 12.5% of the original SO2Cl2 (by moles) has decomposed to reach equilibrium. The total pressure (at equilibrium) is 0.900 atm. Calculate the value of Kp for this system.

###### FREE Expert Solution

We are being asked to calculate Kp for the given reaction:

Balanced reaction:     SO2Cl2(g) SO2(g) + Cl2(g)

When dealing with equilibrium and Kp:

Kp → equilibrium units in terms of pressure
Kp is an equilibrium expression:

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

only gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the pressures in the equilibrium expression

In order to determine the equilibrium concentrations of compounds, we need to use an ICE Chart

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###### Problem Details

At 25ºC, gaseous SO2Cl2 decomposes to SO2(g) and Cl2(g) to the extent that 12.5% of the original SO2Cl2 (by moles) has decomposed to reach equilibrium. The total pressure (at equilibrium) is 0.900 atm. Calculate the value of Kp for this system.