Consider the combustion reaction for octane (C8H18), which is a primary component of gasoline. 2C8H18+25O2⟶16CO2+18H2O

How many moles of CO2 are emitted into the atmosphere when 16.1 g C8H18 is burned?

NEED ASAP PLEASE.

When 16.1 g of octane burn 1.12 moles of  CO₂ are emitted in atmosphere.

Explanation:

Given data:

Mass of octane C₈H₁₈ = 16.1 g

Moles of CO₂ emitted = ?

Solution:

Chemical equation:

2C₈H₁₈ + 25O₂     →    16CO₂+ 18H₂O

Number of moles of octane:

Number of moles = mass/molar mass

Number of moles = 16.1 g/ 114.23 g/mol

Number of moles = 0.14 mol

Now we will compare the moles of octane with carbon dioxide.

             C₈H₁₈            :              CO₂

                 2               :               16

                0.14           :            16/2×0.14 = 1.12 moles

When 16.1 g of octane burn 1.12 moles of  CO₂ are emitted in atmosphere.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

2b2t

explanation:

2b2t