Given the following hypothetical reaction: 2 E(g) + F(g) + G(g) products. If the rate law is: Rate = k[E]2[F]-1, what is the overall order of reaction?
1. a. zero
2. b. first
3. c. second
4. d. third
The order with respect to E is second order, with respect to F is -1 order, the overall over is first (2-1 = 1)
To determine the overall order of the reaction, we need to add up the exponents of each reactant in the rate law.
In this case, the rate law is: Rate = k[E]²[F]⁻¹
The exponents are:
- For reactant E: 2
- For reactant F: -1
To calculate the overall order, we add up the exponents: 2 + (-1) = 1
Therefore, the overall order of the reaction is 1, which means it is a first-order reaction.
The correct answer is b. first.