Question
The rate of a reaction A + 2B --> products is determined. When the concentration of A is 1.0 M, the rate of the reaction is 0.50 M/s. When the concentration of A is 0.50 M, the rate is 0.25 M/s. From this data, you can determine:
a.
that the reaction is second order in A.
b.
that the reaction is 0 order in A.
c.
that the reaction is 1/2 order in A.
d.
that the reaction is first order in A.
e.
nothing about the order of the reaction.
a.
that the reaction is second order in A.
b.
that the reaction is 0 order in A.
c.
that the reaction is 1/2 order in A.
d.
that the reaction is first order in A.
e.
nothing about the order of the reaction.
Answers
DrBob222
rate1 = k1(A)^x
---------------
rate2 = k1(A)^x
You know k1 and k2 are the same so they cancel.
rate1 = 0.50; (A) = 1.0M
rate2 = 0.25; (A) = 0.50
Substitute
0.50 = (1.0)^x
--------------
0.25 = (0.50)^x
Solve.
2 = 2^x
So x must be what?
---------------
rate2 = k1(A)^x
You know k1 and k2 are the same so they cancel.
rate1 = 0.50; (A) = 1.0M
rate2 = 0.25; (A) = 0.50
Substitute
0.50 = (1.0)^x
--------------
0.25 = (0.50)^x
Solve.
2 = 2^x
So x must be what?
Fiona
1.7