Combustion of 8.9541 grams of c4h10 will yield (example 2.345) do not enter units. grams of co2. (assume 100% yield)

The mass of carbon dioxide produced is 27.1 grams.

Explanation:

Combustion reaction is defined as the reaction in which a hydrocarbon reacts with oxygen gas to produce carbon dioxide gas and water molecule.

To calculate the number of moles, we use the equation:

     .....(1)

Given mass of butane = 8.9541 g

Molar mass of butane = 58.12 g/mol

Putting values in equation 1, we get:

The chemical equation for the combustion of butane follows:

By Stoichiometry of the reaction:

2 moles of butane produces 8 moles of carbon dioxide

So, 0.154 moles of butane will produce = of carbon dioxide

Now, calculating the mass of carbon dioxide by using equation 1, we get:

Moles of carbon dioxide = 0.616 moles

Mass of carbon dioxide = 44 g/mol

Putting values in equation 1, we get:

Hence, the mass of carbon dioxide produced is 27.1 grams.

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