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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