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Lesechka [4]
3 years ago
13

If a sample of butene (C4H8) that has a mass of 259.9 g is combusted in excess oxygen, what is the mass of CO2 that is produced?

Chemistry
1 answer:
cluponka [151]3 years ago
6 0
The balanced chemical reaction is expressed as:

<span>C4H8 + 6 O2 ⟶ 4 CO2 + 4 H2O
</span>
To determine the mass of carbon dioxide that is produced from the reaction, we use the initial amount of the limiting reactant which is butene in this case. Also, from the relation of the substances in the reaction we can relate CO2 and the amount of the reactant. We calculate as follows:

moles C4H8 = 259.9 g C4H8 ( 1 mol C4H8 / 56.12 g C4H8 ) = 4.63 mol C4H8
moles CO2 = 4.63 mol C4H8 ( 4 mol CO2 / 1 mol C4H8 ) = 18.52 mol CO2
mass CO2 = 18.52 mol CO2 ( 44.01 g / 1 mol ) = 815.27 g CO2 produced
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5.6 g of solid CO2 is put in an empty sealed 4.00 L container at a temperature of
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Answer:

0.78 atm

Explanation:

Step 1:

Data obtained from the question. This includes:

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Volume (V) = 4L

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Pressure (P) =?

Step 2:

Determination of the number of mole of CO2.

This is illustrated below:

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Step 3:

Determination of the pressure in the container.

The pressure in the container can be obtained by applying the ideal gas equation as follow:

PV = nRT

The gas constant (R) = 0.082atm.L/Kmol

The number of mole (n) = 0.127 mole

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Divide both side by 4

P = (0.127 x 0.082 x 300) /4

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