Question

For the given reaction, what is the correct rate law?
\[ \frac{d[A]}{dt} = -6 \frac{d[B]}{dt} = -4 \frac{d[C]}{dt} = 3 \frac{d[D]}{dt} = 4 \frac{d}{dt} \]

• A. \( 6A + 4B \rightarrow 3C + D \)
• B. \( 3A + 2B \rightarrow 4C + 3D \)
• C. \( 3A + 2B \rightarrow 3C + 4D \)
• D. \( 2A + 3B \rightarrow 4C + 3D \)

Hint:

When writing rate laws, make sure to match the stoichiometric coefficients with the observed reaction mechanism.

Answer 1

The Correct Option is D

Step 1: Understanding the Reaction.
The reaction involves the stoichiometry of the reaction between A, B, C, and D. The rate law should match the correct stoichiometric coefficients.
Step 2: Analyzing the Options.
- (A) \( 6A + 4B \rightarrow 3C + D \) does not match the stoichiometry of the reaction.
- (B) \( 3A + 2B \rightarrow 4C + 3D \) does not match the stoichiometric coefficients.
- (C) \( 3A + 2B \rightarrow 3C + 4D \) is incorrect.
- (D) \( 2A + 3B \rightarrow 4C + 3D \) matches the stoichiometric coefficients, making it the correct answer.
Step 3: Conclusion.
The correct answer is (D) \( 2A + 3B \rightarrow 4C + 3D \).