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CaHeK987 [17]
2 years ago
5

For the reaction represented by the equation Fe + H2O ® Fe2O3 + H2, how many moles of iron(III) oxide are produced from 285 g of

iron? Make sure your equation is balanced.
Chemistry
1 answer:
schepotkina [342]2 years ago
8 0

Balanced equation: 2Fe + 3H2O → Fe2O3 +3H2

Convert g to mols:

285/55.845 = 5.1034 mols

Mole ratio of Iron and Iron (III) Oxide: 2:1

5.1034/2 = 2.5517 mols

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Answer: Option (C) is the correct answer.

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\text{Hg} \text{O} and \text{Hg}_{2} \text{O}.

Assuming complete decomposition of both samples,

  • m(\text{Hg}) = m(\text{residure})
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n = m/M; 0.6498 \; g of the first compound would contain

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Oxygen and mercury atoms seemingly exist in the first compound at a 1:1 ratio; thus the empirical formula for this compound would be \text{Hg} \text{O} where the subscript "1" is omitted.

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