From previous experiments, you have the following information.

N2(g)+O2(g)<--->2NO(g) Kc=2.3*10^-19
2NO(g)+O2(g)<--->2NO2(g) Kc=3*10^6

using that information, how many moles of NO2(g) will be made if you started with 1 moles of N2(g) and 2 moles of O2 (g)?

N2(g)+2O2(g)<--->2NO2(g)

The reaction equation is just the sum of equation 1 and equation 2. Therefore, Kc for the reaction equation is k1*k2 = 6.9E-13

............N2 + 2O2 ==> 2NO2
I...........1.....2.......0
C..........-x....-2x......+2x
E..........1-x..2-2x.......2x
Substitute into Kc expression for the new reaction and solve. You want to find 2x = mols NO2

To determine how many moles of NO2(g) will be produced, we can use the given equilibrium constants (Kc values) and the initial number of moles of reactants.

Let's solve this step by step:

Step 1: Set up the given reactions and conditions.

N2(g) + O2(g) <--> 2NO(g) (1)
2NO(g) + O2(g) <--> 2NO2(g) (2)

The equilibrium constant Kc relates the concentrations of products and reactants at equilibrium. The value of Kc for reaction (1) is 2.3*10^-19, and for reaction (2) is 3*10^6.

Step 2: Determine the initial concentrations of the reactants.

We are given that we start with 1 mole of N2(g) and 2 moles of O2(g).

Step 3: Calculate the concentrations at equilibrium.

For reaction (1), we start with 1 mole of N2 and 2 moles of O2. As the stoichiometry of the reaction dictates, 1 mole of N2 reacts with 1 mole of O2 to produce 2 moles of NO. Since the reaction is at equilibrium, the number of moles of NO is equal to the initial concentration of NO.

For reaction (2), we have 2 moles of NO from the previous step and 2 moles of O2. As the stoichiometry of the reaction dictates, 2 moles of NO reacts with 1 mole of O2 to produce 2 moles of NO2. Thus, the number of moles of NO2(g) is equal to the initial concentration of NO2(g).

Step 4: Calculate the equilibrium concentrations.

Using the given equilibrium constants:
Kc1 = [NO]^2 / ([N2] * [O2])
Kc2 = [NO2]^2 / ([NO]^2 * [O2])

We can rearrange the equations and substitute the given values into the expression to calculate the equilibrium concentrations.

Step 5: Calculate the moles of NO2(g) at equilibrium.

Since the number of moles is equal to the concentration at equilibrium, we can directly use the result we obtained for the equilibrium concentration of NO2(g) in step 4.

Therefore, the moles of NO2(g) formed when starting with 1 mole of N2(g) and 2 moles of O2(g) can be determined by carrying out the calculations outlined above.