When 0.40 moles of PCI, is heated in a 10.0 L container, equilibrium is established is which 0.25 moles of
Cl2 is present. Find Keq PCl5(g) <====> PC13(g) + Cl2(g)
To find Keq, we need to use the equation for the equilibrium constant:
Keq = ([PCl3] * [Cl2]) / [PCl5]
First, we need to find the initial concentrations of the reactants and products.
Given:
Initial moles of PCl5 = 0.40 moles
Initial volume of container = 10.0 L
We can assume that the volume of the container doesn't change during the reaction, so the concentration of PCl5 can be calculated as:
[PCl5] = (moles of PCl5) / (volume of container)
= 0.40 moles / 10.0 L
= 0.04 M
Since PCl3 and Cl2 are both produced in the reaction, we need to calculate their concentrations using stoichiometry.
From the balanced equation:
1 mole of PCl5 produces 1 mole of PCl3 and 1 mole of Cl2
So, the number of moles of PCl3 and Cl2 produced will be equal to the number of moles of PCl5 used. Therefore:
[PCl3] = 0.40 moles / 10.0 L
= 0.04 M
[Cl2] = 0.40 moles / 10.0 L
= 0.04 M
Now we can substitute these values into the equation for Keq:
Keq = ([PCl3] * [Cl2]) / [PCl5]
= (0.04 M * 0.04 M) / 0.04 M
= 0.001 M
Therefore, the value of Keq for the reaction PCl5(g) <====> PCl3(g) + Cl2(g) is 0.001.