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    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
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    (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.
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    (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) ?
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    (Original post by PleaseHelppppp)
    It would be (1.0 + 0.0) ?
    So, what would the amount of product formed be in your hypothetical problem?
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    (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?
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    (Original post by PleaseHelppppp)
    (0+0.7) would be moles reacted + initial moles. So this the answer?
    Huzzah.

    Simples?
 
 
 
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