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Standard XII

Chemistry

Zero Order Reaction

In the Arrhen...

Question

In the Arrhenius equation for a certain reaction, the values of $A$ and $E_{a} a r e 4 \times 10^{13} s^{- 1} a n d 98.6 k J m o l^{- 1}$ , respectively. If the reaction is of first order, the temperature( $i n K$ ) at which its half-time period be 10min is:

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Solution

Half life = $\frac{0.693}{k}$
$o r 10 \times 60 = \frac{0.693}{k}$
$o r k = \frac{0.693}{600}$
Since,
$k = A e^{- E_{a} / R T}$
$l o g k = l o g A - \frac{E_{a}}{2.303 R T}$
or log $\frac{0.693}{600} = l o g 4 \times 10^{13} - \frac{98.6 \times 10^{3}}{2.303 \times 8.314 \times T}$
or $T = 311.35 K$

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In the Arrhenius equation for a certain reaction, the values of A and Eaare4×1013s−1and98.6kJmol−1, respectively. If the reaction is of first order, the temperature(inK) at which its half-time period be 10min is:

Half life = 0.693kor10×60=0.693kork=0.693600Since,k=Ae−Ea/RTlogk=logA−Ea2.303RTor log 0.693600=log4×1013−98.6×1032.303×8.314×Tor T=311.35K

In the Arrhenius equation for a certain reaction, the values of $A$ and $E_{a} a r e 4 \times 10^{13} s^{- 1} a n d 98.6 k J m o l^{- 1}$ , respectively. If the reaction is of first order, the temperature( $i n K$ ) at which its half-time period be 10min is: