- The reaction 2 X + Y →3 Z was studied and the following data were obtained:
Experiment X Y Rate (mole / liter ⋅sec)
1 3.0 1.5 1.8
2 1.5 3.0 0.45
3 1.5 1.5 0.45
What is the proper rate expression?
A. rate = k[X][Y]
B. rate = k[Y]^2
C. rate = k[X]
D. rate = k[X]^2 [Y]
E. rate = k[X]^2
Answer: E
Examine experiments 2 and 3, wherein [X] is held constant. Note that as [Y] doubles (from 1.5
to 3.0), the rate does not change. Hence, the rate is independent of [Y] and the order is 0 for Y.
Now examine experiments 1 and 3, wherein [Y] is held constant. Note that as [X] doubles, the
rate is increased by a factor of 4. In this case, the rate is proportional to the square of the con-
centration of the reactant. This is a second-order reactant.
Combining these reactant orders in a rate equation gives
rate = k[X]^2 [Y]^0 = k[X]^2
For Samples 7 and 8, refer to the following diagram.
Path of Reaction
A
B
C
Energy
Part II: Specific Topics