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Ket [755]
4 years ago
7

What mass of iron would be required to react with 10.0L of O2 gas?

Chemistry
1 answer:
SashulF [63]4 years ago
4 0

33.2 g of iron (Fe)

Explanation:

We have the following chemical reaction in which iron react with oxygen to form the iron (III) oxide:

4 Fe + 3 O₂ → 2 Fe₂O₃

number of moles = volume / 22.4 (L/mole)

number of moles of O₂ = 10 / 22.4

number of moles of O₂ = 0.446 moles

Taking in account the chemical reaction we devise the following reasoning:

if           4 moles of Fe react with 3 moles of O₂

then     X moles of Fe react with 0.446 moles of O₂

X = (4 × 0.446) / 3 = 0.595 moles of Fe

number of moles = mass / molar weight

mass =  number of moles × molar weight

mass of Fe = 0.595 × 55.8

mass of Fe = 33.2 g

Learn more about:

number of moles

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0.8 g H2 (1 mol H2 / 2.02 gH2) (2 mol HCl/1mol H2) ( 36.46 g HCl/1mol HCl) = 28.88 g HCl

 

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If 354.2g PbCl2 are reacted with excess Na3PO4, how many grams of NaCl will be produced
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Answer: The mass of NaCl produced is, 149 grams.

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\text{Moles of }PbCl_2=\frac{\text{Given mass }PbCl_2}{\text{Molar mass }PbCl_2}

\text{Moles of }PbCl_2=\frac{354.2g}{278g/mol}=1.27mol

Now we have to calculate the moles of CaCl_2

The balanced chemical equation is:

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From the reaction, we conclude that

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