Calculate the mass of CO2 produced by the combustion of a tank of gasoline. Assume the mass of gasoline is 46.0 kg and that gasoline is pure octane (C8H18).

142035.09g

Explanation:

Let us write a balanced equation for the reaction. This is illustrated below:

2C8H18 + 25O2 —> 16CO2 +18H2O

Molar Mass of C8H18 = (8x12) + (18x1) = 96 + 18 = 114g/mol

Mass of C8H18 from the balanced equation = 2 x 114 = 228g

Mass of C8H18 from the question = 46kg = 46 x 1000 = 46000g

Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g

Mass of CO2 from the balanced equation = 16 x 44 = 704g

From the equation,

228g of C8H18 produced 704g of CO2.

Therefore, 46000g of C8H18 will produce = (46000 x 704)/228 = 142035.09g of CO2

the correct name for the n3 ion is azide. azide is a polyatomic anion with a -1 charge and is written as n3 -1. it consists of three nitrogen atoms bonded together. hope i . let me know if you need anything else.

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