According to the Arrhenius equation,which of | vedclass

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(C) The Arrhenius equation is given by $k = Ae^{-E_a/RT}$.The rate of reaction is directly proportional to the rate constant $k$.As the temperature $(

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Increase in temperature or decrease in Activation Energy will increase the rate of reaction.

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(C) The Arrhenius equation is given by $k = Ae^{-E_a/RT}$.The rate of reaction is directly proportional to the rate constant $k$.As the temperature $(T)$ increases,the value of the exponent term $-E_a/RT$ becomes less negative (closer to zero),which increases the value of $e^{-E_a/RT}$ and consequently increases $k$.Similarly,as the Activation Energy $(E_a)$ decreases,the exponent term $-E_a/RT$ becomes less negative,which also increases the value of $e^{-E_a/RT}$ and increases $k$.Therefore,increasing the temperature or decreasing the activation energy will increase the rate of reaction.

According to the Arrhenius equation,which of the following statements is correct?

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The variation of the rate constant with temperature is given by the Arrhenius equation $k = A e^{-E_a / (RT)}$. If $T \to \infty$,the rate constant $k$ will be equal to:

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According to the Arrhenius equation,a plot of the logarithm of the rate constant $(\log \, k)$ versus which of the following yields a straight line?

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