# AP CHEM

posted by
**Gabe** on
.

**For the reaction A + 2B + C ----> 2 D + E the following initial concentration and initial reaction rates are found:
[A]null (M) [B]null (M) [C]null (M)
0.150 0.150 0.150
0.275 0.150 0.150
0.275 0.564 0.150
0.150 0.314 0.253
0.193 0.314 0.217
initial rate wrt E (Ms^-1)
0.210
0.285
4.037
0.125
?????
a) find the exponents m n and p of the reactants A B and C
b)what is the overall order to reaction for this reaction?
c)find the rate constant k using experiment 3 including units.
d)find the rate of reaction wrt E for experiment 5**

so far....i've attempted the questions but i'm stuck. here's what i have

rate=k[A]^n[B]^m[C]^p

rate 2/rate 1=

0.285/0.210=k(.275)n(.150)m(.150)p/

k(.150)(.150)(.150)

1.36 = (.275/.150)

1.36 = (1.83)^n

is this correct so far????

thanks in advance