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Goshia [24]
3 years ago
13

A) How much CO is required for the production of Fe from 1000 tonnes of magnetite (Fe2O4). Assume that the iron ore is 100% pure

.
B) How many kilograms of iron should be produced?

C) If the reaction yielded 555 kg of Fe, what is the percentage yield for the process
Chemistry
1 answer:
Kryger [21]3 years ago
5 0
Its b im pretty sure
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Answer:

The combustion of 59.7 grams of methane releases 3320.81 kilojoules of energy

Explanation:

Given;

CH₄ + 2O₂ → CO₂ + 2H₂O, ΔH = -890 kJ/mol

From the combustion reaction above, it can be observed that;

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59.7 g of CH₄ = \frac{59.7}{16} = 3.73125 \ moles

1 mole of methane (CH₄) released 890 kilojoules of energy

3.73125 moles of methane (CH₄) will release ?

= 3.73125 moles x  -890 kJ/mol

= -3320.81 kJ

Therefore, the combustion of 59.7 grams of methane releases 3320.81 kilojoules of energy

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determine the molecular formula of the compound with an empirical formula of CH and a molar mass of 78.110g/mol
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