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Sagot :
Answer:
[tex]\displaystyle K_c \approx 0.0424[/tex]
General Formulas and Concepts:
Math
Pre-Algebra
Order of Operations: BPEMDAS
- Brackets
- Parenthesis
- Exponents
- Multiplication
- Division
- Addition
- Subtraction
- Left to Right
Chemistry
Equilibrium
- Equilibrium Constant K
- Concentrations - Denoted in [Brackets]
Step-by-step explanation:
Step 1: Define
[RxN] 2NO₂ ⇆ N₂O₄
[Equilibrium Rate Law] [tex]\displaystyle K_c = \frac{[N_2O_4]}{[NO_2]^2}[/tex]
NO₂ = 11.95 M
N₂O₄ = 6.05 M
Step 2: Find K
- Substitute [ERL]: [tex]\displaystyle K_c = \frac{[6.05]}{[11.95]^2}[/tex]
- Exponents: [tex]\displaystyle K_c = \frac{[6.05]}{[142.803]}[/tex]
- Divide: [tex]\displaystyle K_c = 0.042366[/tex]
- Round (Sig Figs): [tex]\displaystyle K_c \approx 0.0424[/tex]
This value of K tells us that the reactants are favored in the equilibrium reaction (K < 0.1).
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