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erica [24]
3 years ago
6

A major component of gasoline is octane (C8H18). When octane is burned in air, it chemically reacts with oxygen gas (O2) to prod

uce carbon dioxide (CO2) and water (H2O).
What mass of carbon dioxide is produced by the reaction of 9.88 g of oxygen gas?

Round your answer to 3 significant digits.
Chemistry
1 answer:
Molodets [167]3 years ago
7 0

Answers:

8.70 g

Step-by-step explanation:

We know we will need a balanced equation with masses and molar masses, so let’s <em>gather all the information</em> in one place.  

M_r:                   32.00      44.01

           2C₈H₁₈ + 25O₂ ⟶ 16CO₂ + 18H₂O

m/g:                    9.88

(a) Calculate the <em>moles of O₂ </em>

n = 9.88 g O₂ ×1 mol O₂ /32.00 g O₂

n = 0.3088 mol O₂

(b) Calculate the <em>moles of CO₂</em>

The molar ratio is (16 mol CO₂/25 mol O₂)

n = 0.3088 mol O₂ × (16 mol CO₂/25 mol O₂)

n = 0.1976 mol CO₂

(c) Calculate the <em>mass of CO₂ </em>

Mass of CO₂ = 0.1976 mol CO₂ × (44.01 g CO₂/1 mol CO₂)

Mass of CO₂ = 8.70 g CO₂

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Explanation:

We'll begin by calculating the number of mole in 3.24 g of Mg. This can be obtained as follow:

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Next, we shall write the balanced equation for the reaction. This is illustrated below:

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From the balanced equation above,

1 mole of Mg reacted to produce 1 mole of H2.

Finally, we shall determine the number of mole of H2 produced by reacting 3.24 g (i.e 0.135 mole) of Mg. This can be obtained as follow:

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1 mole of Mg reacted to produce 1 mole of H2.

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Using wolfram alpha or some other reference, determine which of these elements would be liquid at 525 k (assume samples are prot
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