We’re being asked to calculate the overall order of this hypothetical reaction:
2A + B → products
Recall that the rate law only focuses on the reactant concentrations and has a general form of:
$\overline{){\mathbf{rate}}{\mathbf{}}{\mathbf{law}}{\mathbf{=}}{\mathbf{k}}{\left[\mathbf{A}\right]}^{{\mathbf{x}}}{\left[\mathbf{B}\right]}^{{\mathbf{y}}}}$
k = rate constant
A & B = reactants
x & y = reactant orders
We’re going to calculate the overall order for the reaction:
The following data were obtained for the hypothetical reaction 2A + B → products.
[A]_{0} (M) | [B]_{0} (M) | Initial Rate (M/s) | |
1 | 0.2 | 0.1 | 5 |
2 | 0.2 | 0.2 | 20 |
3 | 0.6 | 0.1 | 45 |
What is the overall order of this reaction?
A) 3
B) 1/2
C) 0
D) 4
E) 1