In a first order reaction A---> B the ratio of molar concentration of A and B in the reaction mixture after 100 minute is 1:3. What would be the time needed from the start to have them in the ratio of 1:1?

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In a first order reaction A---> B the ratio of molar concentration of A and B in the reaction mixture after 100 minute is 1:3. What would be the time needed from the start to have them in the ratio of 1:1?

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Answer 1 · 2018-03-09T18:10:30

I don't see how this is even physically possible. If the mol ratio of $A$ to $B$ is $1:1$ , and this reaction is irreversible AS-WRITTEN, you can never have more $B$ than $A$ unless $B$ was manually added, or the reaction goes backwards...

If you really mean $3:1$ , then the start of the reaction had a $4:0$ "ratio", and $100$ minutes later, $"1 mol"$ of $A$ reacts to make $"1 mol"$ of $B$ , giving $3:1$ ... Then $100$ minutes later, $"1 mol"$ of $A$ reacts again to make $"1 mol"$ of $B$ , giving the $2:2$ ratio.

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In a first order reaction A---> B the ratio of molar concentration of A and B in the reaction mixture after 100 minute is 1:3. What would be the time needed from the start to have them in the ratio of 1:1?

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