chemical Kinetics lab what does these graphs represent? write as a disscussion.
ID: 567019 • Letter: C
Question
chemical Kinetics lab
what does these graphs represent? write as a disscussion.
Blue dye cc 0.000015286 Bleach 5%(m/v) 2 Temp ep(K) 1/T t3 av.time vol of bleacvol of Bluedye watertoal vol conc. Of b conc. Of blued rate of reactick InK 5,0278.15 0,003595 1.0 274.15 0.003648 22.0 295.15 0.003388 30.6 303.75 0,003292 43.0 316.15 0,003163 229 324 100 212 330 104 42 35 232 224.3333 319 324.3333 103 102.3333 44 43.33333 10.00 10.00 10.00 10.00 10.00 10.00 10.00 10.00 10 10.00 10.00 10.00 30.00 0.223667 5.09533E-06 2.27132E-08 0.00068379-7.28786 10.00 30.00 0.223667 5.09533E-06 1.57102E-08 0.000472967.6565 .00 30.00 0.223667 5.09533E-06 4.97915E-08 0.001498991 -6.50296 10.00 30.00 0.223667 5.09533E-06 1.17585E-07 0.003539926 -5.64365 0 0.223667 5.09533E-06 1.4983E-07 0.00451167-5.40109 4 34 10.00 30.0 10 InK Determination of Eact 12 0.0035957.28786 13 0.0036487.6565 14 0.003388-6.50296 15 0.003292-5.64365 16 0.003163-5,40109 17 18 Eact 0.0032 0.0033 0.0034 0.0035 0.0036 0.0037 ki/mol yF-4779.2x 9.833 20 23 24 25Explanation / Answer
The experiment on which the given graph is based aims to study the rate of reaction between bleach and blue dye.
The reaction can be given by:
Bleach (sodium hypochlorite) + blue dye ---->products
According to rate law,
rate=k [bleach]^m [blue dye]^n
where m=order of the rxn with respect to bleach
n=order of reaction with respect to blue dye
k=rate constant at a given temperature
Firstly ,
to determine m ,the concentration of blue dye is kept constant,so that,
rate=k [bleach]^m [blue dye]^n=k' [bleach]^m , k'=k[blue dye]^n
or, log rate=log k' +m log [bleach] [type of equation =linear ,form :y=mx +c with slope=m,intercept=log k']
The graph between log rate vs log [bleach] is linear with slope=m
Simiarly, keeping [bleach ] constant,
rate=k [bleach]^m [blue dye]^n=k'' [blue dye]^n , k''=k [bleach]^m
or, log rate=log k'' +n log [blue dye] [[type of equation =linear ,form :y=mx +c with slope=m,intercept=log k'']
A plot of log rate vs log [dye] is linear with slope=n
Thus m,n can be put in any equation like k''=k [bleach]^m with known bleach concentration to calculate k (log k'' can be taken as the intercept)
The topmost graph is based on Arrhenius equation, which relates temperature (T) and rate constant (k), using the equation,
k=A exp(-Eact/RT)
or, ln k=lnA-Eact/RT where Eact=activation energy,R=universal gas constant T=temperature
A plot between lnk and 1/T gives you a inear graph, with slope =-Eact/R from which Eact can be calculated .
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