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
To answer your questions, let's consider the given information and go step by step:
a) Find the exponents m, n, and p of the reactants A, B, and C:
To determine the exponents, we need to compare the ratios of the initial rates with the ratios of the corresponding initial concentrations for each reactant.
Let's compare experiments 2 and 1:
rate 2 / rate 1 = 0.285 / 0.210
[A]null2 / [A]null1 = 0.275 / 0.150
[B]null2 / [B]null1 = 0.150 / 0.150
[C]null2 / [C]null1 = 0.150 / 0.150
From these ratios, we can see that the concentrations of B and C remain constant, while the concentration of A increases. Therefore, the exponent for A (n) is 1, and the exponents for B (m) and C (p) are both 0.
So, the balanced chemical equation is: A + 2B + C -> 2D + E
b) What is the overall order of the reaction?
The overall order of a reaction is the sum of the exponents (n + m + p). In this case, the overall order is 1 + 0 + 0 = 1.
c) Find the rate constant k using experiment 3, including units.
To find the rate constant (k), we need to use one of the experiments that provides values for all the reactant concentrations as well as the initial rate.
Let's use experiment 3:
rate 3 = 4.037 Ms^-1
[A]null3 = 0.275 M
[B]null3 = 0.564 M
[C]null3 = 0.150 M
Plugging these values into the rate equation:
4.037 = k * (0.275)^1 * (0.564)^0 * (0.150)^0
Simplifying:
k = 4.037 / 0.275
k โ 14.66 Ms^-1
Therefore, the rate constant (k) is approximately 14.66 Ms^-1.
d) Find the rate of reaction with respect to E for experiment 5:
To find the rate of reaction with respect to E, we need to compare the ratio of the initial rates with respect to E in different experiments.
Let's compare experiments 5 and 1:
rate 5 / rate 1 = ? / 0.210
[A]null5 / [A]null1 = 0.193 / 0.150
[B]null5 / [B]null1 = 0.314 / 0.150
[C]null5 / [C]null1 = 0.217 / 0.150
Since the experiment does not provide the value for the rate, we cannot calculate the rate of reaction with respect to E for experiment 5.
I hope this helps! Let me know if you have any further questions.