Question

Using the data in the table, determine the rate constant of the reaction and provide the appropriate units.

A+2B⟶C+D

Trial	[?] (?)	[?] (?)	Rate (M/s)
1	0.280	0.380	0.0210
2	0.280	0.760	0.0210
3	0.560	0.380	0.0840

Thank you in advance

Answer 1

see experiment 1 and 3:

[A] doubles

[B] is constant

rate becomes 4 times

so, order of A is 2

see experiment 1 and 2:

[A] is constant

[B] doubles

rate is constant

so, order of B is 0

Rate law is:

rate = k*[A]^2

Put values from 1st row of table in rate law

rate = k*[A]^2

2.1*10^-2 = k*0.28^2*0.38^0

k = 0.2679 M-1.s-1

Answer: 0.268 M-1.s-1