Please explain how to solve for equilibrium concentrations? From week 1 homework

[805751553]

The reaction

N2O4↽−−⇀2NO2

is allowed to reach equilibrium in a chloroform solution at 25 ∘C . The equilibrium concentrations are 0.424 mol/L N2O4 and 2.18 mol/L NO2 .
Kc=11.2


Calculate the equilibrium concentrations of N2O4 and NO2 after the extra 1.00 mol NO2 is added to 1.00 L of solution.

I'm not quite sure how to proceed with the second part of the problem can someone please explain the steps to proceed?

[605775499]

Once you find the E for the first part, you turn those values into the I for the second part but add 1 to the NO2 side.

For example if you got 0.XX and 0.YY as the Equilibrium concentration initially, you'd repeat the table but with 1.XX and 0.YY.