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Equilibria Question help

Basically, when you are working out Kc concentration for products, you do initial moles + moles reacted when given an equilibrium concentration for a reactant, for example.

So if a reactant was 1 mole intially, but 0.3 at equilbrium and you were finding out the equilibrium moles for product, would it be (0+0.3) or (0+0.7) ?
Im getting confused.

Thanks
Reply 1
Avatar for Pigster
Pigster
20
Original post by PleaseHelppppp
So if a reactant was 1 mole intially, but 0.3 at equilbrium and you were finding out the equilibrium moles for product, would it be (0+0.3) or (0+0.7) ?


Assuming a reaction like A <-> B, i.e. 1 mol of reactant turns into 1 mol of product.

Rather than answer your Q, how about I re-quote you with a small change:

Original post by PleaseHelppppp
So if a reactant was 1 mole intially, but 0 at equilbrium and you were finding out the equilibrium moles for product, would it be (0+0) or (0+1.0) ?


I hope you now know which of your suggestions was correct.
Original post by Pigster
Assuming a reaction like A <-> B, i.e. 1 mol of reactant turns into 1 mol of product.

Rather than answer your Q, how about I re-quote you with a small change:



I hope you now know which of your suggestions was correct.


It would be (1.0 + 0.0) ?
Reply 3
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Pigster
20
Original post by PleaseHelppppp
It would be (1.0 + 0.0) ?


So, what would the amount of product formed be in your hypothetical problem?
Original post by Pigster
So, what would the amount of product formed be in your hypothetical problem?


(0+0.7) would be moles reacted + initial moles. So this the answer?
(edited 6 years ago)
Reply 5
Avatar for Pigster
Pigster
20
Original post by PleaseHelppppp
(0+0.7) would be moles reacted + initial moles. So this the answer?


Huzzah.

Simples?

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