Consider the following reaction. 2Fe2O3(s)+3C(s)−→−heat4Fe(s)+3CO2(g) Calculate the number of grams of Fe2O3 needed

Question

Consider the following reaction.

2Fe2O3(s)+3C(s)−→−heat4Fe(s)+3CO2(g)

Calculate the number of grams of Fe2O3 needed to react with 13.0 g C.

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Thạch Thảo 2 weeks 2021-09-05T13:51:04+00:00 1 Answers 0 views 0

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    2021-09-05T13:52:25+00:00

    Answer:

    Number of moles of C = 13.0 g / 12.0107 g/mol = 1.08 mole

    From the balanced equation we can say that

    3 mole of C requires 2 mole of Fe2O3 so

    1.08 mole of C will require

    = 1.08 mole of C *(2 mole of Fe2O3 / 3 mole of C)

    = 0.720 mole of Fe2O3

    mass of 1 mole of Fe2O3 = 159.69 g so

    the mass of 0.720 mole of Fe2O3 = 115 g

    Therefore, the mass of Fe2O3 produced would be 115 g

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Giải phương trình 1 ẩn: x + 2 - 2(x + 1) = -x . Hỏi x = ? ( )