# What Are the Partial Pressures of SO2, Cl2, and SO2Cl2 at Equilibrium?

• suckerpunched
In summary, Sulfuryl chloride SO2Cl2 decomposes into SO2 and Cl2 when heated, with an endothermic reaction. A sample of 3.509 grams of SO2Cl2 was placed into an evacuated 1.00 liter bulb and heated to 375K. At equilibrium, the total pressure was found to be 1.43 atm. Using proportions and an initial, change, equilibrium table, the partial pressures at equilibrium were calculated to be SO2Cl2=0.715 atm, Cl2=0.376 atm, and SO2=0.339 atm. The problem also gave a hint about using an initial, change, equilibrium table to find the equilibrium constant and the effect of increasing
suckerpunched

## 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

okay I am pretty that if you were to take the grams of S02Cl2 and convert that into moles you could use PV=nRT to get the pressure.
Then make your ice chart and that will be the initial pressure of SO2Cl2. And the initial pressures for SO2 and Cl2 would be 0. The change for them would be -x x and x.
so for E you would end with initial pressure SO2Cl2-x x and x.
the problem gives you that the total pressure is 1.43atm so that's the sum of the equilibirum pressures of the ICE chart. You can solve for x and use that to find all the pressures.

.

my response would be that your approach using proportions is incorrect for this problem. The use of an initial, change, equilibrium table is necessary to properly solve this problem. The equilibrium constant can be found using the partial pressures of the reactants and products at equilibrium. The effect of temperature on the equilibrium constant can also be determined using this table. I would recommend reviewing your approach and using the correct equations and methodology for finding partial pressures and equilibrium constants in an equilibrium system.

## What is equilibrium?

Equilibrium refers to a state in which the rate of a forward chemical reaction is equal to the rate of the reverse reaction, resulting in a constant concentration of reactants and products.

## What factors can affect equilibrium?

The factors that can affect equilibrium include temperature, pressure, and the concentration of reactants and products. Changes in any of these factors can shift the equilibrium in favor of either the forward or reverse reaction.

## What is a partial pressure?

Partial pressure is the pressure exerted by an individual gas within a mixture of gases. It is calculated by multiplying the total pressure of the gas mixture by the mole fraction of the individual gas.

## How does partial pressure affect equilibrium?

In a gaseous equilibrium, changes in the partial pressure of any of the gases involved will result in a shift in equilibrium towards the side with a lower partial pressure. This is because the system will try to equalize the partial pressures of the gases.

## How can I calculate partial pressures?

Partial pressures can be calculated using the ideal gas law, which states that the product of pressure and volume is proportional to the number of moles and the temperature of the gas. Alternatively, partial pressures can also be calculated by multiplying the total pressure by the mole fraction of the individual gas.

• Biology and Chemistry Homework Help
Replies
2
Views
16K
• Biology and Chemistry Homework Help
Replies
5
Views
1K
• Biology and Chemistry Homework Help
Replies
19
Views
3K
• Biology and Chemistry Homework Help
Replies
2
Views
2K
• Biology and Chemistry Homework Help
Replies
4
Views
7K
• Biology and Chemistry Homework Help
Replies
2
Views
4K
• Biology and Chemistry Homework Help
Replies
2
Views
9K
• Biology and Chemistry Homework Help
Replies
4
Views
8K
• Biology and Chemistry Homework Help
Replies
2
Views
11K
• Engineering and Comp Sci Homework Help
Replies
7
Views
2K