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3 years ago

What volume of carbon dioxide (CO2) will be produced if 2.90 moles of it on (Fe) is produced?

Chemistry

1 answer:

dolphi86 [110]3 years ago

6 0

Answer:

= 97.44 Liters at S.T.P

Explanation:

The reaction between Iron (iii) oxide and Carbon monoxide is given by the equation;

Fe2O3(s)+ 3CO(g) → 3CO2(g) + 2Fe(s)

From the reaction when the reactants react, 2 moles of Fe and 3 moles of CO2 are produced.

Therefore; Mole ratio of Iron : Carbon dioxide is 2:3

Thus; Moles of Carbon dioxide = (2.9/2)×3

= 4.35 moles

But; 1 mole of CO2 at s.t.p occupies 22.4 liters

Therefore;

Mass of CO2 = 22.4 × 4.35 Moles

= 97.44 L

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2 years ago

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Shkiper50 [21]

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3 years ago

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3 years ago

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3 years ago

In the important industrial process for producing ammonia (the Haber Process), the overall reaction is:

Kisachek [45]

Answer:

Explanation:

Here we have to use stoichiometry.

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1.7 g ------- 98%

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Second, we have to calculate the mass of N2 that is necessary to react to produce the mass of 1.73g of NH3. To do that, we have to use the Molar mass of N2 and NH3 and don't forget the stoichiometric relationship between them.

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3 years ago