I need help. I have no clue how to find this.

A flask is charged with 1.680 atm of N2O4(g) and 1.220 atm of NO2(g) at 25 degrees celcius. The equilibrium reaction is
N2O4 <-> 2 NO2
After equilibrium is reached, the partial pressure of NO2 is 0.550
(a) What is the equilibrium partial pressure of N2O4?
(b) Calculate the Kp for the reaction

I have tried
1.22^2/ 1.680 = 0.550^2/x
but the Webassign said it was wrong. I have also tried
1.220^2/1.680 = 0.886
0.55^2/x = 0.886
x= 2.9289

Note the correct spelling of Celsius.

.........N2O4 <-> 2NO2
I........1.680.....1.220
C.........-p.......+2p
E........1.680-p...2p

The problem tells you that 2p = 0.550. You can calculate p from that.

That allows you to evaluate 1.680-p

Then substitute these values into the Kp expression and evaluate Kp.

To solve this problem, we need to use the concept of equilibrium and the equilibrium constant (Kp). Let's walk through the steps to find the equilibrium partial pressures of N2O4 and the value of Kp.

(a) To find the equilibrium partial pressure of N2O4, we need to set up an expression using the equilibrium constant (Kp) for the reaction: N2O4 <-> 2 NO2.

The equation for Kp is:
Kp = (P(NO2))^2 / P(N2O4)

We are given that the partial pressure of NO2 at equilibrium (P(NO2)) is 0.550 atm. Let's denote the equilibrium partial pressure of N2O4 as P(N2O4).

Using the given values, the equation becomes:
Kp = (0.550)^2 / P(N2O4)

Now, substitute the given equilibrium pressures:
1.680 atm = (0.550)^2 / P(N2O4)

To solve for P(N2O4), rearrange the equation:
P(N2O4) = (0.550)^2 / 1.680

Calculate this expression to find the equilibrium partial pressure of N2O4.

(b) To calculate the value of Kp for the reaction, we'll use the equilibrium partial pressures of N2O4 and NO2.

From part (a), we found that P(N2O4) = (0.550)^2 / 1.680.

Now, use the equilibrium expression for Kp:
Kp = (P(NO2))^2 / P(N2O4)

Substitute the given equilibrium pressures:
Kp = (0.550)^2 / [(0.550)^2 / 1.680]

Simplify this expression by dividing (0.550)^2 on both sides of the fraction:
Kp = 1.680

So, the value of Kp for the reaction is 1.680.

Make sure to recheck your calculations, especially the simplifications, to ensure accuracy.