The reaction A k Products- is zero order while the reaction B k products- is 1st order- for what initial concentration of A the half lives of the two reactions are equal -

The correct option is B 2ℓ n 2 For a first order reaction, the half life is given by: t_1/2 =ln2 k While for a zero order reaction, t_1/2 = a2k So ...

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Standard XII

Chemistry

Half life

The reaction ...

Question

The reaction $A k \to$ Products, is zero order while the reaction $B k \to$ products, is 1st order. for what initial concentration of A the half lives of the two reactions are equal ?

2

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ℓ n 2

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2 log 2

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2 ℓ n 2

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Solution

The correct option is B $2 ℓ n 2$
For a first-order reaction, the half-life is given by:
$t_{1 / 2} = \frac{l n 2}{k}$
While for a zero order reaction,
$t_{1 / 2} = \frac{a}{2 k}$
So, half life of two will be equal when $a = 2 l n 2 =$ initial concentration of A

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The reaction Ak→ Products, is zero order while the reaction Bk→ products, is 1st order. for what initial concentration of A the half lives of the two reactions are equal ?

The correct option is B 2ℓn2For a first-order reaction, the half-life is given by:t1/2=ln2kWhile for a zero order reaction,t1/2=a2kSo, half life of two will be equal when a=2 ln2= initial concentration of A

The reaction $A k \to$ Products, is zero order while the reaction $B k \to$ products, is 1st order. for what initial concentration of A the half lives of the two reactions are equal ?

The correct option is B $2 ℓ n 2$
For a first-order reaction, the half-life is given by:
$t_{1 / 2} = \frac{l n 2}{k}$
While for a zero order reaction,
$t_{1 / 2} = \frac{a}{2 k}$
So, half life of two will be equal when $a = 2 l n 2 =$ initial concentration of A