SO2(g) + NO2(g) reverse reaction arrow SO3(g) + NO (g)

At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M.
---How many moles/liter of NO2 would have to be added to the original equilibrium mixture to increase the equilibrium concentration of SO3 from 3.00 M to 4.10 M at the same temperature?

How would you set this up? I tried to set it up using (4.1)(3.1)/(2.9)(.5+x) = 3, but got it wrong...and also tried (4.1)(2.0+x)/(4.0-1.1)(.5+X)=3...and also got it wrong...

initial:

SO3 = 3.00
NO = 2.00
NO2 = 0.500
SO2 4.00

New equilibrium:
If you want SO3 to be 4.10, that means adding 1.10 to it. Therefore, NO will be 2.00 + 1.10 = 3.30 at new equilibrium.
SO2 = 4.00+x at new eq.
NO2 = 0.500+x at new eq.
Solve for x and don't forget to add the x amount to 4.00 and to 0.500.

i thought you would have to decrease x from SO2?

I think you are right. Let me think about it and get back. I increased BOTH SO2 and NO2 and that isn't the question. I'll be gone about the next hour or so, then I'll get back.

OK. Ate supper, watched the news, thought about the problem and you are absolutely correct. I appreciate you bringing this to my attention. I just didn't think and I increased BOTH reactants. That isn't what the problem asked us to do.

So we make a minor change.
NO = 3.10
SO3 = 4.10
SO2 = 4.00-x
NO2 = 0.500+x
That way we are increasing NO2, which the problem asked us to do, and the SO3 is adjusting itself to whatever value it needs so that the increased amounts of NO2, SO2, and NO will be off-set and Kc still equals 3.00
I obtained x = 0.841 so the new equilibrium amounts should be
SO2 = 4.00-0.841
NO2 = 0.5 + 0.841
NO = 3.10
SO2 = 4.10
I checked Kc and it is 3.00 with these values.

To solve this problem, we need to use the concept of equilibrium constant. The equilibrium constant, Kc, for the given reaction can be expressed as:

Kc = [SO3] * [NO] / [SO2] * [NO2]

We are given the initial concentrations of the species involved in the reaction and the equilibrium concentration of SO3. Let's label the change in concentration of NO2 as x, which we need to find.

Given:
[SO2] = 4.00 M
[NO2] = 0.500 M
[SO3] = 3.00 M
[NO] = 2.00 M
[SO3] (equilibrium) = 4.10 M

Now, let's set up the equation using the equilibrium constant:

Kc = (4.10) * (2.00) / (4.00) * (0.500 + x)

Simplifying this equation:

Kc = 8.20 / (4.00 * 0.500 + 4.00 * x)

Next, we can substitute the expression for Kc using the given value of Kc (which is not provided in the question):

8.20 = (4.10) * (2.00) / (4.00 * 0.500 + 4.00 * x)

Now, we can solve this equation for x by cross-multiplying and simplifying:

8.20 * (4.00 * 0.500 + 4.00 * x) = (4.10) * (2.00)

16.40 + 32.80 * x = 8.20

32.80 * x = 8.20 - 16.40

32.80 * x = -8.20

x = (-8.20) / 32.80

x = -0.25

Since we are looking for the change in concentration of NO2 when increasing the equilibrium concentration of SO3 from 3.00 M to 4.10 M, we can ignore the negative sign. Hence, the change in concentration of NO2, x, is 0.25 M.

To find the moles per liter of NO2, we can simply multiply x by the volume in liters. However, the volume of the original mixture is not given in the question. Therefore, we cannot determine the exact moles per liter of NO2 that needs to be added to the original equilibrium mixture.