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(B) The rate of reaction generally increases with an increase in temperature for most reactions due to an increase in the number of effective collisio

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Increases with increase in temperature

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(B) The rate of reaction generally increases with an increase in temperature for most reactions due to an increase in the number of effective collisions. However,the effect can be complex depending on the reaction mechanism. For a simple elementary reaction,the rate constant $k$ increases with temperature according to the Arrhenius equation,$k = Ae^{-E_a/RT}$. While the rate of reaction typically increases,the statement that it 'may increase or decrease' is sometimes used in specific contexts involving complex mechanisms or reversible reactions where equilibrium shifts significantly. However,in standard chemical kinetics,the rate of reaction is primarily expected to increase with temperature.

$Step$	$Rate\ Constant\ /\ Activation\ energy$
$Step\ 1$	$k_1, E_{a_1} = 180\ kJ/mol$
$Step\ 2$	$k_2, E_{a_2} = 80\ kJ/mol$
$Step\ 3$	$k_3, E_{a_3} = 50\ kJ/mol$

How does the rate of reaction change with an increase in temperature?

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