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A reaction has an activation energy of $209 \mathrm{~kJ}$ $\mathrm{mol}^{-1}$. The rate increases 10 -fold when the temperature is increased from $27^{\circ} \mathrm{C}$ to $\mathrm{X}{ }^{\circ} \mathrm{C}$. The temperature $\mathrm{X}$ is closest to
[Gas constant, $\mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ ]
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[Gas constant, $\mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ ]
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Verified Answer
The correct answer is:
35
$\log _{10}=\frac{209 \times 10^{3}}{2.303 \times 8.314}\left[\frac{1}{300}-\frac{1}{\mathrm{~T}}\right]$
$9.16 \times 10^{-5}=3.33 \times 10^{-3}-\frac{1}{\mathrm{~T}}$
$\mathrm{~T}=308.4 \mathrm{~K}$
or $35^{\circ} \mathrm{C}=\mathrm{X}$
$9.16 \times 10^{-5}=3.33 \times 10^{-3}-\frac{1}{\mathrm{~T}}$
$\mathrm{~T}=308.4 \mathrm{~K}$
or $35^{\circ} \mathrm{C}=\mathrm{X}$
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