For a first-order reaction A→ products

For a first order reactionln[A][A]0=-kt or [A][A]0=e-kt i.e. [A]0(I-α)[A]0=e-kt α=1-e-kt i.e.

For a first-order reaction A→ products

For a first order reactionln[A][A]0=-kt or [A][A]0=e-kt i.e. [A]0(I-α)[A]0=e-kt α=1-e-kt i.e.

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For a first-order reaction $A \to$ products

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a plot of reciprocal of concentration of the reactant versus time is a straight line.

the time taken for the completion of 75% reaction is thrice of half-life time

the pre-exponential factor in the Arrhenius equation has the dimension of time.

the degree of dissociation of reactant is equal to $1 - \exp (- kt) .$

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For a first order reaction

$\ln \frac{[A]}{[A]_{0}} = - k t$ or $\frac{[A]}{[A]_{0}} = e^{- k t}$ i.e. $\frac{[A]_{0} (I - α)}{[A]_{0}} = e^{- k t}$ $α = 1 - e^{- k t}$ i.e.

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For a first-order reaction $A \to$ products