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suckerpunched

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## Homework Statement

Sulfuryl chloride SO2Cl2 decomposes into SO2 and Cl2 when heated. The decomposition is endothermic. A sample of 3.509 grams is placed into an evacuated 1.00 liter bulb and the temp is raised to 375K.

When the system has come to equilibrium at 375K, the total pressure is fount to be 1.43 atm. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium

## Homework Equations

Tried using proportions because no equilibrium constant is given

total mass of 1 mol of each compound: 270.2g

molar mass of 1 mol SO2Cl2: 135.1

molar mass of 1 mol SO2: 64.1

molar mass of 1 mol Cl2: 71.0

1.43atm * part/270.2g= x pressure of part

## The Attempt at a Solution

SO2Cl2=.715atm

Cl2=.376atm

SO2=.339atm

The thing is, we were given the hint that an initial, change, equilibrium table would be needed somewhere in the problem, the other parts being pressure before dissociation, finding the equilibrium constant (part c, this is part b) and finally the effect the temp going to 500K would have on the equilibrium constant