Question

The rate law for the reaction, \(x \mathrm{~A}+y \mathrm{~B} \longrightarrow \mathrm{mP}+\mathrm{nQ}\), is \(\mathrm{r}=\mathrm{k}[\mathrm{A}]^{\mathrm{c}} \times[\mathrm{B}]^{\mathrm{d}}\) What is the overall order of reaction?

• A. \((x+y)\)
• B. \((m+n)\)
• C. \((\mathrm{c}+\mathrm{d})\)
• D. \(\frac{x}{y}\)

Hint:

Overall order is the sum of the powers of concentrations in the experimental rate law.

Answer 1

The Correct Option is C

Step 1: Understanding the Concept
The order of a reaction is determined from the rate law, not from the balanced equation coefficients.

Step 2: Apply to the given law
Rate law: \(r = k[\text{A}]^{c}[\text{B}]^{d}\), so the overall order is the sum of the exponents \(c + d\).

Step 3: Compare the options
Coefficients \(x, y, m, n\) are stoichiometric numbers and do not give the order. Option (C) is correct.

Final Answer:
The overall order of the reaction is c + d. \[ \boxed{\text{(C) }(c+d)} \]