<h3>
Answer:</h3>

<h3>
General Formulas and Concepts:</h3>
<u>Math</u>
<u>Pre-Algebra</u>
Order of Operations: BPEMDAS
- Brackets
- Parenthesis
- Exponents
- Multiplication
- Division
- Addition
- Subtraction
<u>Chemistry</u>
<u>Equilibrium</u>
- Equilibrium Constant K
- Concentrations - Denoted in [Brackets]
<h3>
Step-by-step explanation:</h3>
<u>Step 1: Define</u>
[RxN] 2NO₂ ⇆ N₂O₄
[Equilibrium Rate Law] ![\displaystyle K_c = \frac{[N_2O_4]}{[NO_2]^2}](https://tex.z-dn.net/?f=%5Cdisplaystyle%20K_c%20%3D%20%5Cfrac%7B%5BN_2O_4%5D%7D%7B%5BNO_2%5D%5E2%7D)
NO₂ = 11.95 M
N₂O₄ = 6.05 M
<u>Step 2: Find K</u>
- Substitute [ERL]:
![\displaystyle K_c = \frac{[6.05]}{[11.95]^2}](https://tex.z-dn.net/?f=%5Cdisplaystyle%20K_c%20%3D%20%5Cfrac%7B%5B6.05%5D%7D%7B%5B11.95%5D%5E2%7D)
- Exponents:
![\displaystyle K_c = \frac{[6.05]}{[142.803]}](https://tex.z-dn.net/?f=%5Cdisplaystyle%20K_c%20%3D%20%5Cfrac%7B%5B6.05%5D%7D%7B%5B142.803%5D%7D)
- Divide:

- Round (Sig Figs):

This value of K tells us that the reactants are favored in the equilibrium reaction (K < 0.1).
If i'm correct, the answer should be
-3a
hope this helped! 8)
Answer:
-4
Step-by-step explanation:
2 1/4 - 7 1/2 = -5.25
-5.25 - (-1 1/4) = -4