Half-life period of the first order reaction is 100 days. After 144.3 days, concentration of the reactant is reduced to ldots ldots of the original value.

Question

Half-life period of the first order reaction is 100 days. After 144.3 days, concentration of the reactant is reduced to ldots ldots of the original value. (A) (1/e2) (B) (1/e) (C) 20 % (D) 10 %

Tardigrade Admin · Accepted Answer

T50=(0.693/k) ∴ k=(0.693/t50)=(0.693/100) day -1 (1/k)=(100/0.693)=1.44 .3 days = Average life Thus, given time t=(1/k) (Average life) C = Coe - kt = Coe - k / k =( Co /e) Thus, concentration is reduced to ((1/e)) of the initial value.

Q. Half-life period of the first order reaction is $100$ days. After $144.3$ days, concentration of the reactant is reduced to $\dots\dots$ of the original value.

$\frac{1}{e ^{2}}$

$\frac{1}{e}$

$20%$

$10%$

Q. Half-life period of the first order reaction is 100 days. After 144.3 days, concentration of the reactant is reduced to …… of the original value.

e21​

e1​

20%

10%

T50​=k0.693​ ∴k=t50​0.693​=1000.693​ day −1 k1​=0.693100​=1.44.3 days = Average life Thus, given time t=k1​ (Average life) C=Coe−kt=Coe−k/k=eCo​ Thus, concentration is reduced to (e1​) of the initial value.

Q. Half-life period of the first order reaction is $100$ days. After $144.3$ days, concentration of the reactant is reduced to $\dots\dots$ of the original value.

$\frac{1}{e ^{2}}$

$\frac{1}{e}$

$20%$

$10%$