Question

The rate law for the reaction between catalase and hydrogen peroxide can be written as Rate = k [H2O2]x [catalase]y. A catalase solution of unknown, but constant concentration is prepared. Can the partial order with respect to the peroxide (x) be found using this catalase solution? If so, how would you do it? Describe in detail the steps you would take or show a calculation.

Answer #1

Yes, we can get this

we can apply the initial rate law, in which we use the same catalase concentration and we vary the [H2O2] concnetration, we record the rate of reaction ( initial)

In order to calculate the rate law expression for a A+B reaction, we need to apply Initial Rates Method.

Note that the generic formula goes as follows:

r = k [A]^a [B]^b

Note that if we got at least 3 sets of point, in which we have A and B constant, then we could use:

r1 / r2 = (k1 [A]1^a [B]1^b) / (k2 [A]2^a [B]2^b)

If we assume K1 and K2 are constant, then K1= K2 cancel each other

r1 / r2 = ([A]1^a [B]1^b) / ( [A]2^a [B]2^b)

Then, order according to [A] and [B]

r1 / r2 = ([A]1/[A2])^a * ([B]1/[B]2)^b

If we get two points in which A1 = A2, then we could get B, and vise versa for A...

simply

substitute rate reactions

note that ([B]1/[B]2)^b --> catalse, will be always constant, or 1

the decomposition of hydrogen peroxide
H2O2, is first-order reaction. the half-life
of of reaction is 17.0minutes.
a.) What is the rate constant of the reaction?
b.) If you had a bottle of H2O2, how long
would it take for 80% to decompose?

Hydrogen peroxide can
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according to
BaO2(s)+H2SO4(aq)->BaSO4(s)+H2O2(aq)
How many milliliters of 2.75 M H2SO4(aq) are needed to react
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Hydrogen peroxide can be prepared by the reaction of barium
peroxide with sulfuric acid according to
BaO2(s) + H2SO4(aq) ----> BaSO4(s) + H2O2(aq)
How many milliliters of 4.00 M H2SO4(aq) are needed to react
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The decomposition of hydrogen peroxide (H2O2) is a first order
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20°C?
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(c) How many hours will it take for the concentration to drop to
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0 ,
60 , 120 ,
180 , 240 , 360 , 420 ,
600
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