(8) For the single step reaction: $A+B \rightarrow 2 C+25 k J$
It is determined that the reaction rate doubles when the temperature is raised from $298 \mathrm{~K}$ to $313 \mathrm{~K}$
Choose all the correct answers as to why the increase in temperature causes an increase in the rate.
Choose the graph that best represents the change in reaction conditione
Activation energy $k$ decreased and molocules are able to break existing bonds.
Increasing temperature decreases the kinetic energy of the molecules.
Faster moving molecules collide less frequently with more likelhood of having the correct orientation.
Increasing temperature increases potential energy of the malecules.
Activation enengy $k$ increased and mokccules are able to break exkting bonds
The number of molecules exceeding the actwation energy decreases and are unable to becak existing bonds.
Increasing temperature decreases potential energy of the molecules.
Faster moving molecules collide mare often with more fikdihood of having the correct orientation. The number of molecules exceeding the acthation energy increases and are able to break existing bondk.
Increasing temperature increases the kinetic energy of the molecules.
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Question

(8) For the single step reaction: $A+B \rightarrow 2 C+25 k J$
It is determined that the reaction rate doubles when the temperature is raised from $298 \mathrm{~K}$ to $313 \mathrm{~K}$
Choose all the correct answers as to why the increase in temperature causes an increase in the rate.
Choose the graph that best represents the change in reaction conditione
Activation energy $k$ decreased and molocules are able to break existing bonds.
Increasing temperature decreases the kinetic energy of the molecules.
Faster moving molecules collide less frequently with more likelhood of having the correct orientation.
Increasing temperature increases potential energy of the malecules.
Activation enengy $k$ increased and mokccules are able to break exkting bonds
The number of molecules exceeding the actwation energy decreases and are unable to becak existing bonds.
Increasing temperature decreases potential energy of the molecules.
Faster moving molecules collide mare often with more fikdihood of having the correct orientation. The number of molecules exceeding the acthation energy increases and are able to break existing bondk.
Increasing temperature increases the kinetic energy of the molecules.
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Accepted Answer

***H*** ∻Key Concept∻ ⚹Increasing temperature increases the kinetic energy of the molecules.⚹ ∻Explanation∻ ⚹When the temperature is raised, the average kinetic energy of the molecules increases, which leads to more frequent and energetic collisions. This increases the likelihood that collisions will have sufficient energy to overcome the activation energy barrier, thus increasing the reaction rate.⚹◊How does an increase in temperature affect the rate of a reaction in terms of activation energy and molecular collisions?⍭ Generate me a similar question◊

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