Consider the following balanced equation for the combustion of butane, a fuel often used in lighters....

Consider the following balanced equation for the combustion of butane, a fuel often used in lighters. 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(g) Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed.

Mass C4H10

Mass O2

Mass CO2

Mass H2O

1.31 g

5.12 g

15.12 g

8.44 g

252 mg

168 mg

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Expert Solution

queen_honey_blossom answered 1 year ago

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