# CHEMISTRY PLEASE HELP

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