Question

Given the Table

Trial	[O2]	[H2]	initial rate (M/s)
1	0.128	.231	4.44
2	0.128	.347	6.67
3	.0256	.231	6.28
4	.0102	.462	?

What is the order of this reaction with respect to [O₂]?

a. 0

b. 1/2

c. 1

d. 2

e. 3

My answer key says the answer is b. 1/2, but I have no idea how you get this answer. Everytime I attempted it, I got the answer 0. Can someone explain how you get this answer?

Answer 1

from the table i am sure your trail values are wrong

in third and fourth column concentration of [O2] must be 0.256, 0.102

but you have given 0.0256 , 0.0102 if these vakues are there that table will not follow the chemical kinitics principals

now lets imagine concentrations are 0.256 , 0.102

now while moving from first one to third one

concentration of [O2] doubled rate increased 6.28- (4.44/2) = 2.22

= 4.44 + 2.22 = 6.66

that means rate increased 2.22 times which is exactly half to intial concentration

so order with respect to [O2] is 1/2

so your answer key is correct.