The rate law for the decomposition of aqueous hydrogenperoxide
(h2o2) at 70 degrees celcius is first order in
with k=.0347 min to the negative 1.
a) calculate the half-life (t1/2) for this reaction at
70degrees c
b) given that the initial concentration of h202 is
.300mcalculate the concentration of h2o2 after 60 minutes
haselapsed.

Explanation:

(a)

Given that:

Rate constant, k = 0.0347 min⁻¹

The expression for the half-life is:-

Where, k is rate constant

So,  

(b)

Using integrated rate law for first order kinetics as:

Where,  

is the concentration at time t

is the initial concentration

Given that:

The rate constant, k = min⁻¹

t = 60 min

Initial concentration = 0.300 M

Final concentration =?

Applying in the above equation, we get that:-

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explanation:

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answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.