PLEASE HELP!!

The equilibrium constant is 0.090 at a particular temperature for the reaction:

H2O(g) + Cl2O(g) ⇌ 2HOCl(g)

Use this information to decide what will happen, given the following sets of initial conditions:
Will the reaction shift to the left, to the right or will the system be at equilibrium?

PH2O = 480 torr, PCl2O = 14 torr, PHOCl = 24.6 torr

A 1.0 L flask contains 1.15 mol H2O, 0.078 mol Cl2O and 0.09 mol HOCl.

A 2.0 L flask contains 0.56 mol H2O, 0.0005 mol Cl2O and 0.31 mol HOCl.

PH2O = 198 torr,PCl2O = 64.4 torr, PHOCl = 23 torr

Question

PLEASE HELP!!

The equilibrium constant is 0.090 at a particular temperature for the reaction:

H2O(g) + Cl2O(g) ⇌ 2HOCl(g)


Use this information to decide what will happen, given the following sets of initial conditions: 
Will the reaction shift to the left, to the right or will the system be at equilibrium? 


 PH2O = 480 torr, PCl2O = 14 torr, PHOCl = 24.6 torr

 A 1.0 L flask contains 1.15 mol H2O, 0.078 mol Cl2O and 0.09 mol HOCl.

 A 2.0 L flask contains 0.56 mol H2O, 0.0005 mol Cl2O and 0.31 mol HOCl.

 PH2O = 198 torr,PCl2O = 64.4 torr, PHOCl = 23 torr

cooltowl · Answer

@zepdrix

jfraser · Answer

each different set of conditions allows you to find the $reaction \space quotient$, $Q$, which is calculated exactly the same way as the equilibrium constant. The value of Q will tell you where the reaction currently sits relative to equilibrium

cooltowl · Answer

@Cuanchi

cuanchi · Answer

do you know how to set up the Keq for the reaction? https://www.khanacademy.org/science/chemistry/chemical-equilibrium/equilibrium-constant/v/keq-intuition-mathy-and-not-necessary-to-progress