For the reaction A $\to$ B it has been found that the order of the reaction is zero with respect to A. Which of the following expressions correctly describes the reaction?

K = \frac{2.303}{t} l o g \frac{[A_{0}]}{[A]}

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[A_{0}] - [A] = K t

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t_{1 / 2} = \frac{0.693}{K}

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t_{1 / 2} \propto \frac{1}{[A_{0}]}

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Solution

The correct option is A $[A_{0}] - [A] = K t$
For a zero order reaction, $d [A] = - K d t .$
On integrating this equation between limits,

$[A] = [A]_{0}$ at $t = 0$

$[A] = [A]_{t}$ at $t = t$ , we get $[A_{0}] - [A] = K t$

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For the reaction A → B it has been found that the order of the reaction is zero with respect to A. Which of the following expressions correctly describes the reaction?

The correct option is A [A0]−[A]=KtFor a zero order reaction, d[A]=−Kdt.On integrating this equation between limits, [A]=[A]0 at t=0 [A]=[A]t at t=t, we get [A0]−[A]=Kt

For the reaction A $\to$ B it has been found that the order of the reaction is zero with respect to A. Which of the following expressions correctly describes the reaction?

The correct option is A $[A_{0}] - [A] = K t$
For a zero order reaction, $d [A] = - K d t .$
On integrating this equation between limits,

$[A] = [A]_{0}$ at $t = 0$

$[A] = [A]_{t}$ at $t = t$ , we get $[A_{0}] - [A] = K t$