Question

In the reversible reaction, \[ 2NO_2 \rightleftharpoons \text{N}_2\text{O}_4 \] the rate of disappearance of \( NO_2 \) is equal to:

• A. \( \frac{2k_1}{k_2} [NO_2]^2 \)
• B. \( \frac{k_2}{k_1} [NO_2]^2 \)
• C. \( 2k_1 [NO_2]^2 \)
• D. \( k_2 [NO_2]^2 \)

Hint:

The rate of disappearance of a reactant depends on its concentration raised to the power of its order in the reaction.

Answer 1

The Correct Option is C

Step 1: Rate of disappearance of NO\(_2\).
For the given reversible reaction, the rate of disappearance of \( NO_2 \) is related to the concentration of \( NO_2 \).
Step 2: Conclusion.
Thus, the rate of disappearance of \( NO_2 \) is \( 2k_1 [NO_2]^2 \).
Final Answer: \[ \boxed{2k_1 [NO_2]^2} \]