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Hey guys,
I have a general chemistry question for you regarding temperature effect on rate of reaction. It's not an MCATquestion (it's actually from my gen chem 2 exam that I got back today) but I figure this is the best place for it because I can get a good answer, and it will probably benefit you guys at least a little bit if you're prepping for the MCAT. I know I re-inforce my understanding of concepts when I explain them to someone else.
The rates of most chemical reactions are sensitive to a change in the temperature of the reaction system. The increase in rate as the temperature increases is best explained by
a. an increase in the activation energy
b. a decrease in the activation energy
c. an increase in the collision frequency
d. an increase in the number of high energy molecules
e. a decrease in the collision frequency.
I eliminated choices a and b right off the bat because there's no catalyst or anything present that would affect the activation energy. I also eliminated e as an answer choice because the temperature is increasing so I knew that something would increase. I chose choice C, that the increase in rate as the temp increases is best explained by an increase in the collision frequency. The scantron says that the answer is choice D, that the increase in the rate as the temp increases is best explained by an increase in the number of high energy molecules.
I remember learning and reading that an increase in temperature increases the rate because both C and D happen. I'm probably missing something though and I'm hoping you guys can point it out.
Thanks.
I have a general chemistry question for you regarding temperature effect on rate of reaction. It's not an MCATquestion (it's actually from my gen chem 2 exam that I got back today) but I figure this is the best place for it because I can get a good answer, and it will probably benefit you guys at least a little bit if you're prepping for the MCAT. I know I re-inforce my understanding of concepts when I explain them to someone else.
The rates of most chemical reactions are sensitive to a change in the temperature of the reaction system. The increase in rate as the temperature increases is best explained by
a. an increase in the activation energy
b. a decrease in the activation energy
c. an increase in the collision frequency
d. an increase in the number of high energy molecules
e. a decrease in the collision frequency.
I eliminated choices a and b right off the bat because there's no catalyst or anything present that would affect the activation energy. I also eliminated e as an answer choice because the temperature is increasing so I knew that something would increase. I chose choice C, that the increase in rate as the temp increases is best explained by an increase in the collision frequency. The scantron says that the answer is choice D, that the increase in the rate as the temp increases is best explained by an increase in the number of high energy molecules.
I remember learning and reading that an increase in temperature increases the rate because both C and D happen. I'm probably missing something though and I'm hoping you guys can point it out.
Thanks.