Question

For the reaction, \(\text{NO}_{2(g)}+\text{CO}_{(g)}\rightarrow \text{NO}_{(g)}+\text{CO}_{2(g)}\) the rate expression is found to be: rate \(=k[\text{NO}_{2}]^{2}\). What is the order of reaction with respect to CO?

• A. \(2\)
• B. \(0\)
• C. \(1\)
• D. \(1/2\)

Hint:

The order for a reactant is its exponent in the experimental rate law, and CO does not appear in it.

Answer 1

The Correct Option is B

Step 1: Understanding the Concept
The order with respect to a reactant is the power of its concentration in the experimental rate expression.

Step 2: Read the rate law
The given rate is \(\text{rate}=k[\text{NO}_{2}]^{2}\). This can be written as \(k[\text{NO}_{2}]^{2}[\text{CO}]^{0}\).

Step 3: Conclusion
The exponent of \([\text{CO}]\) is 0, so the reaction is zero order in CO. It is second order overall.

Final Answer:
The order with respect to CO is 0. \[ \boxed{\text{(B) }0} \]