Chemistry, 03.12.2019 01:31 PONBallfordM89

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=3.010^6m^-1s^-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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Answer from: kalbaugh

Answer :

The rate of the reaction at t=0 is, $9.0\times 10^{-13}M.s^{-1}$

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:

$A+B\rightarrow C+D$

The general rate law expression for the reaction is:

$\text{Rate}=k[A]^a[B]^b$

where,

a = order with respect to A

b = order with respect to B

R = rate law

k = rate constant

[A] and [B] = concentration of A and B reactant

Now we have to determine the rate law for the given reaction.

The given balanced equations is:

$O_3(g)+NO(g)\rightarrow O_2(g)+NO_2(g)$

In this reaction, O_3 and are the reactants.

The rate law expression for the reaction is:

$\text{Rate}=k[O_2][NO]$ ..........(1)

Given :

Rate constant = $k=3.0\times 10^{-5}M^{-1}s^{-1}$

Concentration of O_3 = $5.0\times 10^{-4}M$

Concentration of = $6.0\times 10^{-5}M$

Now put all the given values in equation 1, we get:

$\text{Rate}=(3.0\times 10^{-5}M^{-1}s^{-1})\times (5.0\times 10^{-4}M)\times (6.0\times 10^{-5}M)$

$\text{Rate}=9.0\times 10^{-13}M.s^{-1}$

Thus, the rate of the reaction at t=0 is, $9.0\times 10^{-13}M.s^{-1}$

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 O_3 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.

Answer from: Quest

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

Answer from: Quest

It conforms what ever surface its in.

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The reaction described by this equation

o3(g)+no(> o2(g)+no2(g)

has th...

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