Intermediate  [ENDORSED]


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William Lan 2l
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Intermediate

Postby William Lan 2l » Thu Mar 08, 2018 12:05 am

How do you determine the intermediate?

Nina Gautam 1K
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Re: Intermediate

Postby Nina Gautam 1K » Thu Mar 08, 2018 8:44 am

As Lavelle said in class, if there are intermediate steps, he will give us the intermediate species. We don't have enough general chemistry knowledge at this point to come up with it on our own.

Elizabeth Bamishaye 2I
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Re: Intermediate

Postby Elizabeth Bamishaye 2I » Thu Mar 08, 2018 9:17 am

Intermediates are the species that are not in overall reaction. You could find them by viewing a species that is produced then it is consumed.

Ya Gao
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Re: Intermediate

Postby Ya Gao » Thu Mar 08, 2018 6:58 pm

Intermediate can be determined by looking at the separate steps of a reaction. If one molecule is produced in one step and consumed in the following step, then the molecule can be considered an intermediate.

Swetha Sundaram 1E
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Re: Intermediate

Postby Swetha Sundaram 1E » Thu Mar 08, 2018 7:17 pm

Right so when you compare them in separate reactions, we essentially cancel them out which is why they are not shown in the final reaction equation.

Sohini Halder 1G
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Re: Intermediate

Postby Sohini Halder 1G » Thu Mar 08, 2018 7:47 pm

Intermediates are FORMED and then CONSUMED within the steps of elementary reactions.
Catalysts are present from the beginning and are not consumed in the reaction; this is why only a little bit of catalyst is needed to increase the rate of a specific reaction.

Ashley Macabasco 2K
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Re: Intermediate

Postby Ashley Macabasco 2K » Thu Mar 08, 2018 8:03 pm

Intermediates are formed in one step and the consumed in the next, so the intermediate will be the species that is present in the steps but not present in the final equation.

Garret G 2F
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Re: Intermediate  [ENDORSED]

Postby Garret G 2F » Sat Mar 10, 2018 5:50 pm

Sohini Halder 1G wrote:Intermediates are FORMED and then CONSUMED within the steps of elementary reactions.
Catalysts are present from the beginning and are not consumed in the reaction; this is why only a little bit of catalyst is needed to increase the rate of a specific reaction.


Here is a video that explains this in a little more detail: https://youtu.be/UkoImD80-BM


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