Consider the following reaction:

2SO2(g) + O2(g) <-> 2SO3(g)

Kp=0.355 at 950 K

A 2.75 L reaction vessel at 950 K initially contains 0.100 mol of SO2 and 0.100 mol of O2.

Calculate the total pressure (in atmospheres) in the reaction vessel when equilibrium is reached.

So, I think I am going to make an ice table:

| SO2 | O2 | SO3 |

Initial Concentration | 0.036 M | 0.036 M | ? |

Change in Concentration | | | |

Equilibrium Concentration | | | |

I got the initial concentrations of SO2 and O2 by dividing the number of mols by 2.75 L

But how do you know the initial concentration of SO3?

I used this equation: Kp=Kc/[(RT)^delta n] to find Kc and found it to be 0.00454

Where do I go from here? I am mainly stuck on the initial concentration of SO3.

Or do I even need to find that? I don't know what I should do.

Thanks!!!