Calculate the pressures of NO, Cl2, and NOCl in an equilibrium mixture produced by the reaction of a starting mixture with 8.2 atm NO and 4.1 atm Cl2. (Hint: Kp is relatively large; assume the reaction goes to completion then comes back to equilibrium.)

The given question is incomplete. The complete question is as follows.

Calculate the pressures of NO, , and NOCl in an equilibrium mixture produced by the reaction of a starting mixture with 8.2 atm NO and 4.1 atm . (Hint: KP is small; assume the reverse reaction goes to completion then comes back to equilibrium.)

Explanation:

According to the ICE table,

Initial:      8.2              4.1              0

Change:    -4.1x           -x               +4.1x

Equilbm: (8.2 - 4.1x)   (4.1 - x)        +4.1x

Now, expression for of the reaction is as follows.

                   x = 1.9

Therefore, at equilibrium

    [NOCl] = = 3.8

    [NO] = (8.2 - 7.79) = 0.41

    = 2 - 1.9 = 0.1        

that's what i got you can count the number of atoms