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xxgissellexx
03.12.2019 •
Chemistry
The reaction described by this equation
o3(g)+no(> o2(g)+no2(g)
has the following rate law at 310k.
rate of reaction=k[o3][no] k=3.0*10^6m^-1*s^-1
given that [o3]=5.0x10^-4m and no=6.0x10^-5m at t=0 calculate the rate of the reaction at t=0
what is the overall order of this reaction?
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Ответ:
Answer :
The rate of the reaction at t=0 is,![9.0\times 10^{-13}M.s^{-1}](/tpl/images/0400/1843/f8d67.png)
The overall order of reaction is, second order reaction.
Explanation :
Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.
The general reaction is:
The general rate law expression for the reaction is:
where,
a = order with respect to A
b = order with respect to B
R = rate law
k = rate constant
Now we have to determine the rate law for the given reaction.
The given balanced equations is:
In this reaction,
and
are the reactants.
The rate law expression for the reaction is:
Given :
Rate constant =![k=3.0\times 10^{-5}M^{-1}s^{-1}](/tpl/images/0400/1843/c49a2.png)
Concentration of
= ![5.0\times 10^{-4}M](/tpl/images/0400/1843/77f5c.png)
Concentration of
= ![6.0\times 10^{-5}M](/tpl/images/0400/1843/b48af.png)
Now put all the given values in equation 1, we get:
Thus, the rate of the reaction at t=0 is,![9.0\times 10^{-13}M.s^{-1}](/tpl/images/0400/1843/f8d67.png)
Now we have to determine the overall order of reaction.
From the given rate law expression we conclude that,
The order of reaction with respect to
is, first order reaction.
The order of reaction with respect to
is, first order reaction.
Thus, overall order of reaction will be:
Overall order of reaction = 1 + 1 = 2
Thus, the overall order of reaction is second order reaction.
Ответ:
increase
Explanation: