The data below were colected for the following reaction: CH3Cl(g) + 3Cl(g) --> C
ID: 790409 • Letter: T
Question
The data below were colected for the following reaction:
CH3Cl(g) + 3Cl(g) --> CCl4(g) + 3HCl(g)
Rate= k[CH3Cl][3Cl]^1/2
Calculate the value of the rate constant, k.
AND
What is the overall order of the reaction?
[CH3Cl] (M) [Cl2] (M) Initial Rate (M/s) 0.050 0.050 0.014 0.100 0.050 0.029 0.100 0.100 0.041 0.200 0.200 0.115Explanation / Answer
the first thing is to find the rate law. to do this you need to take a look at how the rate changes as each of the concentrations of the reactants changes independent of the other.
CH3Cl - 0.1/0.05 = 2 and 0.029/0.014 = 2.07 or ~ 2
so 2^x = 2 which means x = 1. therefore the rxn is first order in CH3Cl
Cl2 - 0.1/0.05 = 2 and 0.041/0.029 = 1.41
so 2^y = 1.41 which means y = 0.5. therefore the rxn is half order in Cl2
this makes the rate law: rate = k[CH3Cl][Cl2]^0.5
1. so the overall order of the rxn is 1.5
2. to find the rate constant, all you need to do is plug in a concentration and its rate and solve for k
0.041 = k[0.100][0.100]^0.5
k = 1.30
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