In: Chemistry
answer
rate = k[NOC]2;
k = 8.0 × 10−8 L/mol/s;
second order
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Where M
and
rate1 are the concentration and rate of one experiment
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and M2 and rate2 are the concentration and rate of another.
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ratio of the respective rates for the NOCl concentrations.
3.2*10^−9 / 8*10^−10==4 :
this shows that the rate is being quadrupled
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From above
NOCl concentration is doubled, the rate is quadrupled.
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have to determine what it takes in order for the doubling of the concentration to quadruple the rate:
2^x==4
solving for x, we find that x=2,
meaning the NOCl is second order.
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Let us assume Experiment 1 uses .3 M and
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Experiment 2 uses .2 M:
7.2*10^−9 /3.2*10^−9=2.25
= 0.3 /0.2 =1.5
We find that the rate order of NOCl remains two:
1.5^2=2.25
Therefore the rate equation is rate= k [NOCl]^2
s there NOCl is the only reactant, the sum of the exponents of the reactants is two and, therefore, the order for this equation is a second order.
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sing the rate law found above, we can use the rate at a given concentration of NOCl to find the rate constant, k.
8.0⋅10^−10(Mh)=k [0.1M]^2
8.0⋅10^−10(Mh)=k [0.1M]^2
solving for k,
k= 8.0 × 10^−8 /M⋅hour
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In order to determine the units for k consider the units for the rate and the concentration:
M/h=M^2⋅x
and thus:
x=M/M^2⋅h=1/M⋅h
Molarity is squared due to the rate order of NOCl being two.
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