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Standard XII

Chemistry

Half life

For the given...

Question

For the given reaction,
$A_{1} K_{2} B$
Where $K_{1}$ is zero order rate constant and $K_{2}$ is first rate constant. The concentration of $B$ at any time can be given by the experssion:

K_{1} = \frac{1}{t} l o g_{10} \frac{[B_{0}]}{[B]}

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K_{1} = \frac{2.303}{t} l o g_{10} \frac{[B_{0}]}{[B]}

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\frac{- 1}{K_{2}} [l o g \frac{l o g K_{1} - K_{2} [B_{0}]}{K_{1} - K_{2} [B]}] = t

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Solution

The correct option is B $K_{1} = \frac{2.303}{t} l o g_{10} \frac{[B_{0}]}{[B]}$
$K_{2}$ is 1st rate constant. So Its a 1st order reaction.So,

$K_{1} = \frac{2.303}{t} l o g \frac{[B_{0}]}{[B]}$

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For the given reaction,AK1⇌K2BWhere K1 is zero order rate constant and K2 is first rate constant. The concentration of B at any time can be given by the experssion:

The correct option is B K1=2.303tlog10[B0][B]K2 is 1st rate constant. So Its a 1st order reaction.So,K1=2.303tlog[B0][B]

For the given reaction,
$A_{1} K_{2} B$
Where $K_{1}$ is zero order rate constant and $K_{2}$ is first rate constant. The concentration of $B$ at any time can be given by the experssion:

The correct option is B $K_{1} = \frac{2.303}{t} l o g_{10} \frac{[B_{0}]}{[B]}$
$K_{2}$ is 1st rate constant. So Its a 1st order reaction.So,

$K_{1} = \frac{2.303}{t} l o g \frac{[B_{0}]}{[B]}$