calculate the number of pounds of co2 released into the atmosphere when a 25.0 gallon tank of gasoline is burned in an automobile engine. assume that gasoline is primarily octane, c8h18, and that the density of gasoline is 0.692 g⋅ml−1. this assumption ignores additives. also, assume complete combustion. co2 released: lb

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aryanagarwal466 aryanagarwal466 · Answer 1 · 2022-09-11T09:20:02+02:00

445.616 lb of CO2.

Equation for the reaction:

C8H18 + 25/2O2(g) --> 8CO2(g) + 9H2O(g)

Given:

The volume of gasoline = 25gallon

Converting gallon to ml,

25 gallon * 3.785 l/1 gallon * 1000 ml/1 l

= 94,625 ml

Density of the gasoline = 0.692 g/ml

Mass = density * volume

= 94,625 * 0.692

= 65480g

Molar mass of octane = (8*12) + (18*1)

= 114 g/mol.

Number of moles = mass/molar mass

= 65480/114

= 574.390 mol.

From the above equation, 1 mole of octane was completely burnt to give off 8 moles of CO2.

By stoichiometry,

Number of moles of CO2 = 574.390* 8

= 4595.122 mol of CO2.

Molar mass of CO2 = 12 + (2*16)

= 44 g/mol

Mass of CO2 = number of moles * molar mass

= 4595.122 * 44

=202,185.40 g

Converting g to pound,

= 202,185.40 g *1 kg/1000 g * 2.204 lb/1kg

= 445.616 lb of CO2.

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