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Answer: The mass of carbon dioxide required is 308 g

Step-by-step explanation:

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

The equation used is:


\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}} ......(1)

Given mass of octane = 100.0 g

Molar mass of octane = 114.23 g/mol

Putting values in equation 1, we get:


\text{Moles of octane}=(100.0g)/(114.23g/mol)=0.875mol

For the given chemical reaction:


2C_8H_(18)+25O_2\rightarrow 16CO_2+18H_2O

By the stoichiometry of the reaction:

2 moles of octane produces 16 moles of carbon dioxide

So, 0.875 moles of octane will produce =
(16)/(2)* 0.875=7mol of carbon dioxide

Molar mass of carbon dioxide = 44 g/mol

Plugging values in equation 1:


\text{Mass of carbon dioxide}=(7mol* 44g/mol)=308g

Hence, the mass of carbon dioxide required is 308 g

User Joris Kinable
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