The following data was obtained for the reaction 2A + B ---> 2D @ 25 degrees celsius. What is the rate law expression for the reaction?
Experiment 1, initial [A] was .500, initial [B] was .400, and the initial rate of formation D was 6 X 10 to the -3.
Experiment 2, initial [A] was .250, initial [B] was .400, and the initial rate of formation D was 1.5 X 10 to the -3.
Experiment 3, initial [A] was .250, initial [B] was .800, and the initial rate of formation D was 3 X 10 to the -3.
How do I solve this? I took a sick day from class, we have this for homework tonight, and I need to get this prob to understand the homework. Any cool tricks are appreciated. Thanks in advance.
2007-05-31 10:47:20 · 3 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
the general formula is:
rate=k[A]^m[B]^n
use the data given to solve for k, m, and n
using exp. 1 and 2:
6E-3 = k[.5]^m[.4]^n
1.5E-3=k[.25]^m[.4]^n
Then divide the two equations to cancel out two varibles so that you can solve for the third. You end up with:
4=.5^m / .25^m
4=(.5/.25)^m
4=2^m
m=2
use the same method to solve for n
exp. 2 and 3
3E-3 = k[.25]^m[.8]^n
1.5E-3=k[.25]^m[.4]^n
2=.8^n / .4^n
2=(.8/.4)^n
2=2^n
n=1
you can now use n and m to find k using only the data from one experiment (I'll use exp. 1)
6E-3=k(.5)^2(.4)^1
6E-3 = .1k
k= .06
the final rate law is:
rate = .06[A]^2[B]^1
2007-05-31 11:38:28 · answer #1 · answered by hawkeye3772 4 · 1⤊ 0⤋
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Rate law expression question...?
The following data was obtained for the reaction 2A + B ---> 2D @ 25 degrees celsius. What is the rate law expression for the reaction?
Experiment 1, initial [A] was .500, initial [B] was .400, and the initial rate of formation D was 6 X 10 to the -3.
Experiment 2, initial [A] was .250,...
2015-08-17 01:20:54 · answer #4 · answered by Anonymous · 0⤊ 0⤋
Compare 1 and 2. [A] halves, and [B] is kept constant. The rate shrinks to a quarter, therefore the reaction is second order in A.
Compare 2 and 3. [A] is kept constant, and [B] doubles, and so does the rate. Therefore it is 1st order in B.
Third order overall.
2007-05-31 10:57:53 · answer #5 · answered by Gervald F 7 · 0⤊ 0⤋
Rate = k x [NO2]^2 x [CO] i am pretty sure
2016-03-14 13:39:35 · answer #6 · answered by Anonymous · 0⤊ 0⤋