A reaction has an activation energy of 209 kJ mol -1- The rate increases 10 fold when the temperature is increased from 27- C to X - C- The temperature X - C is closest to- Gas constant- -R -8-314 J mol -1 K -1-A- 35B- 40C- 30D- 45

The correct option is A 35Using Arrhenius equation, ln10=E_aR(1T_1 1T_2) ⇒ 2.303=209 × 10^38.314 (1300 1T_2) ⇒ 9.16 × 10^ 5=1300 1T_2 ⇒ T_2= 308.4 K ⇒ X=35 ^ ...

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Byju's Answer

Standard XII

Chemistry

Rate Constant

A reaction ha...

Question

A reaction has an activation energy of $209 k J m o l^{- 1}$ . The rate increases 10 fold when the temperature is increased from $27^{o} C$ to $X^{o} C$ . The temperature $X^{o} C$ is closest to:
[Gas constant, $R = 8.314 J m o l^{- 1} K^{- 1}$ ]

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Solution

The correct option is A 35
Using Arrhenius equation,
$l n 10 = \frac{E_{a}}{R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$

$\Rightarrow 2.303 = \frac{209 \times 10^{3}}{8.314} (\frac{1}{300} - \frac{1}{T_{2}})$
$\Rightarrow 9.16 \times 10^{- 5} = \frac{1}{300} - \frac{1}{T_{2}}$
$\Rightarrow T_{2} = 308.4 K$

$\Rightarrow X = 35^{o} C$

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A reaction has an activation energy of 209 kJ mol–1. The rate increases 10 fold when the temperature is increased from 27 oC to X oC. The temperature X oC is closest to: [Gas constant, R=8.314 J mol–1 K–1 ]

The correct option is A 35Using Arrhenius equation, ln10=EaR(1T1−1T2) ⇒2.303=209×1038.314(1300−1T2) ⇒9.16×10−5=1300−1T2 ⇒T2=308.4 K ⇒X=35 oC

A reaction has an activation energy of $209 k J m o l^{- 1}$ . The rate increases 10 fold when the temperature is increased from $27^{o} C$ to $X^{o} C$ . The temperature $X^{o} C$ is closest to:
[Gas constant, $R = 8.314 J m o l^{- 1} K^{- 1}$ ]