The energy of activation and specific rate constant for a first order reaction at 25-C are 100kJ-mole and 3-46-10-5sec-1 respectively- Determine the temperature at which half-life of the reaction is 2 hours-

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Standard XII

Chemistry

Rate of Reaction

The energy of...

Question

The energy of activation and specific rate constant for a first order reaction at $25^{\circ}$ C are 100kJ/mole and $3.46 \times 10^{- 5} s e c^{- 1}$ respectively. Determine the temperature at which half-life of the reaction is 2 hours:

306 k

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310 k

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234 k

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280 k

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Solution

The correct option is A 306 k
As we know,
$k = 0.693 / t_{1 / 2} = 0.693 / 2 = 0.3465 / h r$
and $E_{a} = 100$ kJ/mole
$k = A e^{- E_{a} / R T}$ so T is 306K.

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The energy of activation and specific rate constant for a first order reaction at 25∘C are 100kJ/mole and3.46×10−5sec−1 respectively. Determine the temperature at which half-life of the reaction is 2 hours:

The correct option is A 306 kAs we know,k=0.693/t1/2=0.693/2=0.3465/hrand Ea=100kJ/molek=Ae−Ea/RT so T is 306K.

The energy of activation and specific rate constant for a first order reaction at $25^{\circ}$ C are 100kJ/mole and $3.46 \times 10^{- 5} s e c^{- 1}$ respectively. Determine the temperature at which half-life of the reaction is 2 hours:

The correct option is A 306 k
As we know,
$k = 0.693 / t_{1 / 2} = 0.693 / 2 = 0.3465 / h r$
and $E_{a} = 100$ kJ/mole
$k = A e^{- E_{a} / R T}$ so T is 306K.