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:

Kp=productsreactants

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.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the ICE Chart concept. You can view video lessons to learn ICE Chart. Or if you need more ICE Chart practice, you can also practice ICE Chart practice problems.

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Based on our data, we think this problem is relevant for Professor Gulacar's class at UCD.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.