Answer:
The answer is 671 litres of carbon dioxide is produced from 0.410 kg of hexane
Explanation:
We first write a balanced reaction for the complete combustion of hexane thus
The stoichiometry of the cumbustion of hexane in air is
2C6H14(g)+18O2(g)→12CO2(g)+14H2O(l) or
C6H14(g)+9O2(g)→6CO2(g)+7H2O(l)
From the above reaction it is observed that one mole of hexane burns completely in the presence of oxygen to produce 6 moles of carbon dioxide
Therefore we calculate the nuber of moles of hexane present in the sample thus
Mass hexane of sample = 0.41 kg
Molar nass of hexane = 86.18 g/mol
number of moles of hexane = (mass of hexane)/(molar mass of hexane) = (0.41×1000)/86.16 = 410/86.16 = 4.76 moles
As we have seen from the chemical reaction, 1 mole of H6H14 produces 6 moles of CO2 hence 4.76 moles of Hexane produces
4.76×6 moles of CO2 which is 28.55 moles of CO2
From the question we have the temperature and the pressure of the production of CO2 as
Temperature of reaction = 13°
C converting to kelving gives= 13+273.15 = 286.15 K
and pressure = 1 atmosphere or 101325 Pa
13.0∘C=13.0∘C+273.15=286.15 K
The volume of the produced CO2 can be calculated using the combined ideal gas equation given by
P×V=n×R×T where
Here
P = Gas pressure (of CO2
)
V = Volume (of the CO2)
n = number of moles of gas (CO2) present
R = universal gas constant, equal to 0.0821 atm× L/(mol× K
)
T = absolute temperature in Kelvin
Thus we have
1×V = 28.55×0.0821×286.15 or V = 670.76L
Rounding up the answer to 3 significant digits we have
670.76L ≅ 671L
671 litres of carbon dioxide is produced from 0.410 kg of hexane
