Introduced into a 1.50L container is 0.100mol PCl5(g). The flask is held at 227degreesC until equilibrium is established. What are the partial pressures and the total pressures of the gases in the flask at the equilibrium. PCl5(g)<-->PCl3(g)+Cl2(g)
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Well that would be Chemistry, possibly AP Chemistry.
To determine the partial pressures and total pressure at equilibrium, we need to use the information provided and apply the principles of the ideal gas law and equilibrium expressions.
First, let's convert the given volume of the container to liters: 1.50 L.
Next, let's calculate the initial number of moles for each gas species:
- PCl5(g) is initially 0.100 mol.
- Since PCl3(g) and Cl2(g) are not present initially, their initial moles are zero.
Now, to determine the partial pressures at equilibrium, we need to know the equilibrium concentrations of PCl5, PCl3, and Cl2. These can be calculated using the equilibrium constant expression.
The equilibrium constant expression for the given reaction is: K = [PCl3][Cl2] / [PCl5]
where [PCl3], [Cl2], and [PCl5] represent the equilibrium concentrations of PCl3, Cl2, and PCl5, respectively.
Since the equilibrium concentrations are not given, we need more information to calculate them. We can use the ideal gas law to relate the number of moles to pressure and volume:
PV = nRT
Rearranging the equation, we get:
P = nRT / V
We can use this equation to find the partial pressures of PCl3 and Cl2 at equilibrium.
First, let's calculate the total number of moles at equilibrium:
The initial total number of moles is 0.100 mol PCl5. Since PCl3 and Cl2 are formed from PCl5, their number of moles will be equal once equilibrium is reached.
Therefore, the total number of moles at equilibrium is (0.100 mol PCl5 + 0.100 mol PCl3 + 0.100 mol Cl2) = 0.300 mol.
Now, let's calculate the partial pressures:
Partial pressure of PCl5 = (0.100 mol / 0.300 mol) * (nRT / V)
Partial pressure of PCl3 = (0.100 mol / 0.300 mol) * (nRT / V)
Partial pressure of Cl2 = (0.100 mol / 0.300 mol) * (nRT / V)
Finally, to find the total pressure at equilibrium, we need to add up the partial pressures:
Total pressure = Partial pressure of PCl5 + Partial pressure of PCl3 + Partial pressure of Cl2
This will give us the partial pressures of each gas species and the total pressure of the gases in the flask at equilibrium.