[whitefloss]

Consider the following equilibrium: 2NO + O2 = 2NO2
In an experiment, 0.30 mol of NO and 0.80 mol of NO2 are placed in a 5.0L container at 10C. When equilibrium is reached, it is found that (O2) = 0.020M. Calculate Kc.

I have tried making an ice table with 0.30/5M as the initial state of NO as well as 0.80/5M as the initial state for NO2 on the product side. I also wrote 0.020M for the equilibrium state for O2. I am usually only familiar working with ICE tables that have either a 0 for initial reactants or products and a known change amount, or final amount. In this scenario, I am unsure how to figure out the change as well as the equilibrium amount for NO and NO2 since both products and reactants start with some unknown quantity that isn't 0. 

Side Note: I posted the same question yesterday but I did not know how to modify or delete the post so sorry about that.

[chenbeier]

Consider how much NO₂ decompose and how much NO you get if you obtain 1 O₂. Calculate this with the given numbers.

[whitefloss]

Are you saying the product is going to be 0 at equilibrium? I'm still quite confused.

[Borek]

Side Note: I posted the same question yesterday but I did not know how to modify or delete the post so sorry about that.

Then you should continue the discussion in the old thread, not start another one. Consider reading the forum rules that you agreed to while registering.

Everything you need can be calculated just by following the stoichiometry of the reaction, that's what the C row is about.