The rate constant of a reaction increases by five times on increase in temperature from 27-C to 52o- The value of activation energy in kJ mol-1 is - Rounded-off to the nearest integerTake -log10 5-0-7R - 8-314 J K-1 mol-1-

Expression for rate constant at two different temperature is given by nbsp; logK_2K_1 =E_a2.303 R [1T_1 TT_2] log 5 =E_a2.303 × 8.314 [1300 1325] nbsp; ...

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Standard XI

Economics

Shapes of Average and Marginal Cost Curves in the Short Run

The rate cons...

Question

The rate constant of a reaction increases by five times on increase in temperature from $27^{\circ} C t o 52^{o}$ . The value of activation energy in $k J m o l^{- 1}$ is _________. (Rounded-off to the nearest integer)
Take $[l o g_{10} 5 = 0.7 R = 8.314 J K^{- 1} m o l^{- 1}]$

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Solution

Expression for rate constant at two different temperature is given by

$l o g \frac{K_{2}}{K_{1}} = \frac{E_{a}}{2.303 R} [\frac{1}{T_{1}} - \frac{T}{T_{2}}]$

$l o g 5 = \frac{E_{a}}{2.303 \times 8.314} [\frac{1}{300} - \frac{1}{325}]$

$E_{a} = \frac{0.7 \times 2.303 \times 8.314 \times 300 \times 325}{25} J m o l^{- 1}$

$= 52271 J = 52.271 k J m o l^{- 1} = 52$

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The rate constant of a reaction increases by five times on increase in temperature from 27∘C to 52o. The value of activation energy in kJ mol−1 is _________. (Rounded-off to the nearest integer) Take [log105=0.7R=8.314 J K−1 mol−1]

Expression for rate constant at two different temperature is given by logK2K1=Ea2.303 R[1T1−TT2] log 5=Ea2.303×8.314[1300−1325] Ea=0.7×2.303×8.314×300×32525J mol−1 =52271 J=52.271 kJ mol−1=52

The rate constant of a reaction increases by five times on increase in temperature from $27^{\circ} C t o 52^{o}$ . The value of activation energy in $k J m o l^{- 1}$ is _________. (Rounded-off to the nearest integer)
Take $[l o g_{10} 5 = 0.7 R = 8.314 J K^{- 1} m o l^{- 1}]$