Question

2A + B → C

Select the rate law for the reaction above using the following information:

Holding the concentration of A constant and doubling the concentration of B results in the rate of the reaction increasing from 1.5E-3 M/s to 6.0E-3 M/s.
Keeping the concentration of B constant and doubling A results in the rate of the reaction increasing from 1.5E-3 M/s to 3.0E-3 M/s.

A) rate = k [A] [B]2

B) rate = k [A]2 [B]2

C) rate = k [A]2 [B]

D) rate = k [A]2

E) rate = k [B]2

F) rate = k [B]

Answer 1

@timo86m Is it C?

Answer 2

lemme think its been a while :)

Answer 3

Okay @timo86m

Answer 4

Keep in mind that i haven not done this in so long
rate=[A]^a [B]^b

2A+B->C

1st scenerio
1.5 to 6 is 4 with B doubled
2A+2B->6

2nd scenerio
1.5 to 3 is 2 with A doubled
4A+2B-> .5

NOW use that in

[A]^a [B]^b



We can see that B is ^2 and A is 1

Answer 5

I say A. The problem is worded oddly.

Answer 6

but get a second opinion. I am no student of chemistry. I am an autodidact.