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The given chemical reaction is:

\[ 4 \text{NO}(g) + 3 \text{O}_2(g) \rightleftharpoons 2 \text{N}_2\text{O}_5(g) \]

To find the equilibrium constant expression \( K_c \), we use the general form of the equilibrium law for a reaction of the type:

\[ aA + bB \rightleftharpoons cC + dD \]

The equilibrium constant expression is given by:

\[ K_c = \frac{[\text{C}]^c [\text{D}]^d}{[\text{A}]^a [\text{B}]^b} \]

### Applying to the Given Reaction
For the reaction provided:

- \( a = 4 \), for NO
- \( b = 3 \), for \( \text{O}_2 \)
- \( c = 2 \), for \( \text{N}_2\text{O}_5 \)

The equilibrium constant expression \( K_c \) will be:

\[ K_c = \frac{[\text{N}_2\text{O}_5]^2}{[\text{NO}]^4 [\text{O}_2]^3} \]

Now, let's check the options in the image:

1. \(\frac{[\text{N}_2\text{O}_5]}{[\text{NO}][\text{O}_2]^2}\)
2. \(\frac{[\text{N}_2\text{O}_5]^2}{[\text{NO}]^4 [\text{O}_2]^3}\)
3. \(\frac{[\text{NO}]^4}{[\text{N}_2\text{O}_5]^2 [\text{O}_2]}\)
4. \(\frac{[\text{N}_2\text{O}_5]}{[\text{NO}]^2 [\text{O}_2]^3}\)
5. \(\frac{[\text{N}_2\text{O}_5]^2}{[\text{NO}]^4 [\text{O}_2]^2}\)

The correct option is the second one:

\[ K_c = \frac{[\text{N}_2\text{O}_5]^2}{[\text{NO}]^4 [\text{O}_2]^3} \]

Would you like me to explain in more detail or have any other questions?

### Related Questions:
1. What is the difference between \( K_c \) and \( K_p \)?
2. How do temperature changes affect the value of \( K_c \)?
3. What is the significance of the equilibrium constant being greater than 1?
4. How does the reaction quotient \( Q \) compare to \( K_c \)?
5. How can you calculate \( K_c \) if given concentrations at equilibrium?

**Tip:** Always ensure to balance the chemical equation before determining the equilibrium constant expression.

Which of the following expressions is the equilibrium law for the reaction given below? 4NO(g) + 3O2(g) ↔ 2N2O5(g)

Understand how to write the equilibrium constant expression for the reaction 4NO + 3O2 ↔ 2N2O5. This example explores the application of equilibrium laws, showing how to calculate Kc using concentrations of products and reactants. Ideal for high school chemistry students.

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