What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200 K to 400 K? ($R=8.314\ \text{JK}^{-1}\text{mol}^{-1}$) (a) $234.65\ \text{kJ mol}^{-1}$ (b) $434.65\ \text{kJ mol}^{-1}$ (c) $2.305\ \text{kJ mol}^{-1}$ (d) $334.65\ \text{J mol}^{-1}$

What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200 K to

Choose the Best Answer · Q11

R=8.314\ \text{JK}^{-1}\text{mol}^{-1}

(a)

234.65\ \text{kJ mol}^{-1}

(b)

434.65\ \text{kJ mol}^{-1}

(c)

2.305\ \text{kJ mol}^{-1}

(d)

334.65\ \text{J mol}^{-1}

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Step 1. Use the two-temperature Arrhenius form: $\ln\dfrac{k_2}{k_1}=\dfrac{E_a}{R}\left(\dfrac{1}{T_1}-\dfrac{1}{T_2}\right)$ , with $k_2/k_1=2$ (rate doubles), $T_1=200$ K, $T_2=400$ K.

Step 2. $\dfrac{1}{T_1}-\dfrac{1}{T_2}=\dfrac{1}{200}-\dfrac{1}{400}=\dfrac{2-1}{400}=\dfrac{1}{400}\ \text{K}^{-1}$ . …

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Q.What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200 K to 400 K? ( $R=8.314\ \text{JK}^{-1}\text{mol}^{-1}$ )

Concept understanding — Arrhenius Equation and Activation Energy

Q.What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200 K to 400 K? (R=8.314 JK−1mol−1R=8.314\ \text{JK}^{-1}\text{mol}^{-1}R=8.314 JK−1mol−1)

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Q.What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200 K to 400 K? ( $R=8.314\ \text{JK}^{-1}\text{mol}^{-1}$ )

Unlock everything free for 14 days