Into a 1.00 liter flask are placed 0.820 moles of NO and 0.223 moles of N2 and O2. What are the concentrations of NO, N2, and O2 at equilibrium?

For the molarity for each, I got this:
NO= .027 M
N2= .0079 M
O2= .0069 M

balanced equation: 2NO(g) <-> N2(g) + O2
How do I know which side it shifts to? Do I just add up the molarity for each side and make it shift to the lesser value?

Wait, I messed up the values! instead of dividing the moles by 1.00 L, I divided by the molecular weight on accident. I still need help with this problem.

You don't have an equilibrium constant.

M = mols/L; therefore, the mols listed = M.

To determine the shift in the equilibrium of a reaction, you need to compare the initial concentrations with the equilibrium concentrations based on the balanced equation and the reaction quotient, Q.

In this case, the balanced equation for the reaction is:
2NO(g) ↔ N2(g) + O2(g)

The initial concentrations are:
[NO] = 0.820 moles / 1.00 L = 0.820 M
[N2] = [O2] = 0.223 moles / 1.00 L = 0.223 M

To calculate the equilibrium concentrations, you need to figure out the change in moles for each species. Let's assume x moles of NO reacts, which means 2x moles of N2 and O2 are formed. Therefore, the equilibrium concentrations will be:

[NO] = 0.820 M - x M
[N2] = 0.223 M + 2x M
[O2] = 0.223 M + 2x M

Now, you can substitute these equilibrium concentrations into the expression for the reaction quotient, Q:

Q = ([N2] * [O2]) / [NO]^2

Q = [(0.223 + 2x) * (0.223 + 2x)] / [(0.820 - x)^2]

To determine the direction of the shift in the equilibrium, you need to compare Q with the equilibrium constant, K. If Q < K, the reaction will shift to the right (towards the products). If Q > K, the reaction will shift to the left (towards the reactants).

However, you have not provided the value of K for this reaction. If you have the value of K, you can compare it with the calculated value of Q to determine the shift in the equilibrium.

Conversely, if you are given the pressures or partial pressures of the gases instead of molar concentrations, you can still follow the same steps by using the ideal gas law to convert between the two.

Once you have determined the shift in the equilibrium, you can calculate the final concentrations of NO, N2, and O2 by solving the equilibrium equation using the given conditions and the equilibrium concentrations you arrived at.