Question

For the current reaction, 2NO2 ↔ N2O4, we have:

Kc =
`([N_(2) O_(4)])/([NO_(2)]^(2) )`

Concentration of NO2 = 11.95
Concebtration of N2O4 = 6.05
Based on the current concentrations of NO2 and N2O4, what is Kc?

Answer 1

`\displaystyle K_c \approx 0.0424`

General Formulas and Concepts:

Math

Pre-Algebra

Order of Operations: BPEMDAS

1. Brackets
2. Parenthesis
3. Exponents
4. Multiplication
5. Division
6. Addition
7. Subtraction

• Left to Right

Chemistry

Equilibrium

• Equilibrium Constant K
• Concentrations - Denoted in [Brackets]

Explanation:

Step 1: Define

[RxN] 2NO₂ ⇆ N₂O₄

[Equilibrium Rate Law]
`\displaystyle K_c = ([N_2O_4])/([NO_2]^2)`

NO₂ = 11.95 M

N₂O₄ = 6.05 M

Step 2: Find K

1. Substitute [ERL]:
   `\displaystyle K_c = ([6.05])/([11.95]^2)`
2. Exponents:
   `\displaystyle K_c = ([6.05])/([142.803])`
3. Divide:
   `\displaystyle K_c = 0.042366`
4. Round (Sig Figs):
   `\displaystyle K_c \approx 0.0424`

This value of K tells us that the reactants are favored in the equilibrium reaction (K < 0.1).