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10 March, 21:45

If 4.0 moles of X and 4.0 moles of Y react according to the hypothetical reaction below, how many moles of the excess reactant will be left over at the end of the reaction? 2X + 3Y yields X2Y3

1.3 mol Y left over

2.7 mol Y left over

1.3 mol X left over

2.7 mol X left over

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Answers (1)
  1. 10 March, 23:37
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    2X + 3Y - - > X2Y3

    You have initially 4 moles of both X and Y.

    2 moles of X and 3 moles of Y are needed to make X2Y3.

    4 moles X * (3 moles Y/2 moles X) = 6 moles Y

    We do not have 6 moles of y, which means that Y is the limiting reactant.

    4 moles Y * (2 moles X/3 moles Y) = 2.667 moles X

    We start off with 4 moles of X, and we react 2.667 moles of X.

    We start off with 4 moles of Y, and we react all 4 moles of Y. (Remember, this is the limiting reactant.)

    The reactant that will be in excess is X, and it will have 4 - 2.667 = 1.333 moles of X remaining.

    Your final correct answer is 1.3 mol X left over.
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