The rate of reaction increases with temperature due to:

decrease in activation energy

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increase in activation energy

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increase in collision frequency

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none of these

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Solution

The correct option is C increase in collision frequency

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Similar questions

Which of the following statements are in accordance with the Arrhenius equation?
(a) Rate of a reaction increases with increase in temperature
(b) Rate of a reaction increases with a decrease in activation energy
(c) Rate constant decreases exponentially with an increase in temperature
(d) Rate of reaction decreases with a decrease in activation energy

Q. Assertion :A rate of reaction of most of the reactions doubles, when temperature increased from

298 K

308 K

. Reason: The activation energy of reaction decreases with increase in temperature.

Consider the Arrhenius equation given below and mark the correct option.
$k = A . e - \frac{E_{a}}{R T}$
(a) Rate constant increases exponentially with increasing activation energy and decreasing temperature
(b) Rate constant decreases exponentially with increasing activation energy and decreasing temperature
(c) Rate constant increases exponentially with decreasing activation energy and decreasing temperature
(d) Rate constant increases exponentially with decreasing activation energy and increasing temperature

Q. Assertion :According to Von't Hoff's rule, metabolic activity doubles with every

10^{o} C

increase in temperature.
Reason: The reaction rate is not affected with every

10^{o} C

decrease in temperature.

Q. Assertion: The overall rate of a reversible reaction may decrease with the increase in temperature.
Reason: When the activation energy of a forward reaction is less than that of its backward reaction, then the increase in the rate of the backward reaction is more than that of the forward reaction on increasing the temperature.

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