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Tasya [4]
3 years ago
9

F a sample of butene (C4H8) that has a mass of 136.6 g is combusted in excess oxygen, what is the mass of CO2 that is produced?

Chemistry
2 answers:
alukav5142 [94]3 years ago
7 0

The balanced chemical reaction will be:

C4H8 + 6 O2 --> 4 CO2 + 4 H2O

We are given the amount of butene being combusted. This will be our starting point.

136.6 g C4H8 (1 mol  C4H8/ 56.11 g C4H8) (4 mol CO2/1 mol <span>C4H8</span>) ( 44.01 g CO2/ 1 mol CO2) = 428.6 g CO2
swat323 years ago
3 0

Answer : The mass of CO_2 produced will be, 429.264 grams

Explanation : Given,

Mass of C_4H_8 = 136.6 g

Molar mass of C_4H_8 = 56 g/mole

Molar mass of CO_2 = 44 g/mole

First we have to calculate the moles of C_4H_8.

\text{Moles of }C_4H_8=\frac{\text{Mass of }C_4H_8}{\text{Molar mass of }C_4H_8}=\frac{136.6g}{56g/mole}=2.439moles

Now we have to calculate the moles of CO_2.

The balanced chemical reaction is,

C_4H_8+6O_2\rightarrow 4CO_2+4H_2O

From the balanced reaction we conclude that

As, 1 mole of C_4H_8 react to give 4 moles of CO_2

So, 2.439 moles of C_4H_8 react to give \frac{4}{1}\times 2.439=9.756 moles of CO_2

Now we have to calculate the mass of CO_2.

\text{Mass of }CO_2=\text{Moles of }CO_2\times \text{Molar mass of }CO_2

\text{Mass of }CO_2=(9.756mole)\times (44g/mole)=429.264g

Therefore, the mass of CO_2 produced will be, 429.264 grams.

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Explanation:

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Explanation:

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Therefore, putting the given values into the above formula as follows.

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