Answer:
Rate = k [X]⁻¹ [Z]²
Explanation:
[X] [Y] [Z] initial rate M M M M · s −1
Exp 1 0.30 0.20 0.35 0.210
Exp 2 0.60 0.10 0.70 0.420
Exp 3 0.60 0.20 0.70 0.420
Exp 4 0.60 0.40 0.35 0.105
In Experiment 2 and 3 where the concentrations of Y and Z were constant, doubling the concentration of Y had no effect on the rate of the reaction. This means, that the rate of the reaction is zero order with respect to Y.
In experiment 3 and 4, dividing the concentration of Z by 2, causes the rate of the reaction to decrease by 4. This means the rate of the reaction is second order with respect to Z.
In experiment 1 and 4, doubling the concentration of X, causes the rate of the reaction to decrease by half. This means that X has an order of -1 with respect to the rate of the reaction.
The rate expression is given as;
Rate = k [X]⁻¹[Y]⁰[Z]²
Rate = k [X]⁻¹ [Z]²
