intermediate
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intermediate
How are you able to tell what the intermediate is and why can't it exist in the rate law?
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Re: intermediate
An intermediate is a species that is formed and subsequently used up in a reaction mechanism. It can't appear in the rate law because it is not part of the overall reaction.
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Re: intermediate
The intermediate can't exist in the rate law because something was used to form it. So since it came from something, you gotta trace it back to the original components.
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Re: intermediate
Intermediates are produced in one elementary step and consumed in the next. They are not part of the overall reaction so they will not appear in the rate law.
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Re: intermediate
Intermediates are form and then used up so they are not part of the overall reaction and therefor rate law as well
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Re: intermediate
If an intermediate is formed during a reaction, and then used, do non-state functions include those changes and quantities?
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Re: intermediate
The intermediate in a series of reactions can be identified by seeing which element is both in the products of one reaction and reactants of another (it will cancel out as they are on opposite sides). Since it is not written in the overall reaction (as it is cancelled out), it is not included in the rate law equation.
Re: intermediate
Intermediates are easily recognizable in a reaction mechanism, which is the sequence of elementary reactions to go from reactants to products. The molecules that are formed and consumed in these elementary reactions are intermediates
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Re: intermediate
Intermediates ultimately get canceled out when you write out chemical equations in the full, so they will not show up in the rate law because only the initial reactants and final products have an influence on the rate law.
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Re: intermediate
An intermediate is formed and used up during the reaction, so it will not be included in the rate law because it isn't part of the overall reaction.
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Re: intermediate
Intermediates are produced then consumed, during some part of the reaction. It cannot exist in rate law because they are not a part of the overall equation.
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Re: intermediate
An intermediate is formed and then used up during a reaction, so it cant be used in rate law.
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Re: intermediate
The intermediate can't exist in the rate law because something was used to form it.
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Re: intermediate
It is not in the rate law because it was formed then used and does not appear in the overall reaction.
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Re: intermediate
An intermediate was formed (and then used up) by the reaction, so it doesn't show up in the rate law.
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Re: intermediate
The intermediate is both formed and consumed in the reaction but does not appear in the overall chemical equation.
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Re: intermediate
Intermediates are formed in one reaction and then consumed in the other, so they do not show up in rate laws.
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Re: intermediate
The intermediate is formed and used up, and it doesn't appear in the overall chemical equation
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Re: intermediate
An intermediate shows up in the products of step one but the reactants of step two and therefore is used up in the second reaction so none will remain after the whole thing is over. The reason this does not affect the rate law is because the rate law is determined by the reactants of the slow step and the intermediate has no effect on this.
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Re: intermediate
An intermediate will appear in one of the step and be used up in a subsequent step. It will not show up in the overall reaction.
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Re: intermediate
The intermediate cancels out in the rate determining step (before the final overall equation), and is not present in the overall reaction --> as its presence in the reactant of one reaction and the product of another reaction, makes itself cancel out.
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Re: intermediate
Since an intermediate cancels out, you wouldn't write it in the final balanced equation.
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Re: intermediate
An intermediate is produced in the steps of reactions, but it will be the reactant for some follow-up chemical equations and is eventually canceled out after summing all the steps together to get the final formula.
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Re: intermediate
An intermediate will be the product of one elementary reaction and the reactant of another.
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Re: intermediate
Intermediates are formed during the reaction and then used up, so they are not a part of the rate law.
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