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#### Question

The rate constant of a first order reaction increases from 4 × 10^{−2} to 8 × 10^{−2} when the temperature changes from 27°C to 37°C. Calculate the energy of activation (Ea). (log 2 = 0.301, log 3 = 0.4771, log 4 = 0.6021)

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#### Similar questions

The rate constant for the first-order decomposition of H_{2}O_{2} is given by the following equation:

`logk=14.2-(1.0xx10^4)/TK`

Calculate E_{a} for this reaction and rate constant k if its half-life period be 200 minutes.

(Given: R = 8.314 JK^{–1} mol^{–1})

The decomposition of hydrocarbon follows the equation *k *= (4.5 × 10^{11 }s^{−1}) e^{−28000 }^{K}^{/}^{T}

Calculate *E*_{a}.

(b) Rate constant ‘k’ of a reaction varies with temperature ‘T’ according to the equation:

`logk=logA-E_a/2.303R(1/T)`

Where E_{a} is the activation energy. When a graph is plotted for `logk Vs. 1/T` a straight line with a slope of −4250 K is obtained. Calculate ‘E_{a}’ for the reaction.(R = 8.314 JK^{−1} mol^{−1})

The rate constant of a first order reaction increases from 2 × 10^{−2} to 4 × 10^{−2} when the temperature changes from 300 K to 310 K. Calculate the energy of activation (E_{a}).

(log 2 = 0.301, log 3 = 0.4771, log 4 = 0.6021)

What will be the effect of temperature on rate constant?