The volume of CO2 produced from the combustion reaction is 93.73 L at STP.
The balanced combustion reaction of C3H8 with excess oxygen is shown below. Due to the presence of excess oxygen, it is assumed that the reaction would achieve complete combustion. This means that there would be no CO (carbon monoxide) present in the product.
C3H8 + 5O2 → 3CO2 +4H2O
The amount of carbon dioxide can be determined through the use of a stoichiometric ratio with the limiting reactant, C3H8.
To convert the mass of C3H8 to moles, the equation below is used. (Molar mass of C3H8= 44.097 g/mol)
Moles of C3H8= Mass of C3H8 / molar mass of C3H8
Moles of C3H8= 61.5 g / 44.097 g/mol
Moles of C3H8= 1.39465 mol
Then, determine the number of moles of CO2 produced. Every mole of C3H8 reacted produces 3 moles of CO2.
Moles of CO2 = Mole C3H8 * ( 3 mol CO2 / 1 mol C3H8)
Moles of CO2= 4.18396 mol
Lastly, the ideal gas equation, shown below, can be used to calculate the volume of CO2 at STP. The conditions at STP are 1 atm pressure and 273K temperature. (Gas constant=0.082057 L-atm/K-mol)
(Pressure)(Volume)=(number of moles)(gas constant)(temperature)
Volume= [(4.18396 mol)( 0.082057 L-atm/K-mol)(273 K)]/ 1 atm
Volume=93.727 L
The volume of CO2 produced can also be identified by multiplying the number of moles by 22.4016 L/mol, which is the value of volume/number of moles in STP.
For more information regarding combustion reactions, please refer to brainly.com/question/9913173.
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