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cestrela7 [59]
2 years ago
6

Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Fe2O3 are formed when 1.47 g of Fe reacts

completely with oxygen?
Chemistry
1 answer:
ozzi2 years ago
8 0

Answer:

2.10 g

Explanation:

Write the unbalanced reaction:

Fe + O₂ → Fe₂O₃

Balance it:

4Fe + 3O₂ → 2Fe₂O₃

Now use stoichiometry.  Convert mass of Fe to moles of Fe:

1.47 g Fe × (1 mol Fe / 55.8 g Fe) = 0.0263 mol Fe

Convert moles of Fe to moles of Fe₂O₃:

0.0263 mol Fe × (2 mol Fe₂O₃ / 4 mol Fe) = 0.0132 mol Fe₂O₃

Finally, convert moles of Fe₂O₃ to mass of Fe₂O₃:

0.0132 mol Fe₂O₃ × (159.7 g Fe₂O₃ / mol Fe₂O₃) = 2.10 g Fe₂O₃

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When 21.45 g of KNO3 was dissolved in water in a calorimeter, the temperature fell from 25.00°C to 14.14 °C. If the heat capacit
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25.9 kJ/mol. (3 sig. fig. as in the heat capacity.)

<h3>Explanation</h3>

The process:

\text{KNO}_3\;(s) \to \text{KNO}_3\;(aq).

How many moles of this process?

Relative atomic mass from a modern periodic table:

  • K: 39.098;
  • N: 14.007;
  • O: 15.999.

Molar mass of \text{KNO}_3:

M(\text{KNO}_3) = 39.098 + 14.007 + 3\times 15.999 = 101.102\;\text{g}\cdot\text{mol}^{-1}.

Number of moles of the process = Number of moles of \text{KNO}_3 dissolved:

\displaystyle n = \frac{m}{M} = \frac{21.45}{101.102} = 0.212162\;\text{mol}.

What's the enthalpy change of this process?

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\displaystyle \Delta H = \frac{Q}{n} = \frac{5.4843\text{kJ}}{0.212162\;\text{mol}} = 25.8\;\text{kJ}\cdot\text{mol}^{-1}.

The heat capacity is the least accurate number in these calculation. It comes with three significant figures. As a result, round the final result to three significant figures. However, make sure you keep at least one additional figure to minimize the risk of rounding errors during the calculation.

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