Question

The two common chlorides of Phosphorus, PCl3 and PCl5, both important in the production of other phosphorous compounds, coexist in equilibrium through

PCl3 (g) + Cl2 (g)------> PCl5 (g)

At 250 C, an equilibrium mixture in a 2.50 L flask contains 0.105 g PCl5, 0.220 g PCl3, and 2.12 g Cl2.

Show the equilibrium Constant formula

What are the values of (a) Kc for this reaction?

Answer 1

kc = [Molarity Products 1]/[Molarity of reactant 1][Molarity of reactant 2]

Answer 2

You should know how to find the molarity of each of the compounds and if that is not the case then there may be another formula you can use to find the Kc which i do not remember but should be easily available from your chemistry resources

Answer 3

The other formulas may involve using the temperature of the compounds so if it does then do not forget to convert the temperature to Kelvins.

Answer 4

Molarity is equal to moles / liter

Answer 5

And since you know the total Volume in liters of all the products and reactants together then you can find the Molarity of each of the compounds by first finding the moles of each compound and then using the moles to find the molarity

Answer 6

You will need your periodic table to look up the values for each of the compounds which will be in the form of g/mole and since you are given the grams of each of the compounds you can solve for moles by dividing (g/mole) / (g) which will give you moles and then you can use that for molarity which is moles/ liter

Answer 7

oh ok Thank you!

Answer 8

No problem