Question

The half-life of a first order reaction is 0.5 min at a certain temperature. Calculate

(a) the rate constant of the reaction

(b) the time required for 80 % reactant to decompose.​

Answer 1

Answer:

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Explanation:

Decomposition of hydrogen peroxide is 1st Order reaction. So,

t  1/2  =   0.693 /k

k=  0.5 /0.693

​k=1.

B) if it would be 75%

Order of reaction = 1

Let the initial concentration be [A]0 = 100

[A]t = 100 -75 = 25

Rate law for first order rection

K = (2.303/t)log[A]0/[A]t

Substituting the values we get

K = 0.0231

And

t1/2 = 0.693/K = 30 min

sorry i am not able  to solve of 80% but instead of that i solve for 75%