1.50 mol C3H8 X (3 mol CO2 / 1 mol C3H8) X (44.0 g CO2 / 1 mol CO2) = 198 g CO2
The mass of carbon dioxide produced by burning 1.5 mol of propane has been 198.045 grams.
The balanced chemical equation for the reaction has been:
[tex]\rm C_3H_8\;+\;5\;O_2\;\rightarrow\;3\;CO_2\;+\;4\;H_2O[/tex]
According to the balanced equation, in the presence of abundant oxygen, 1 mole of propane, there has been a production of 3 moles of carbon-di-oxide.
The given moles of propane have been 1.50 moles. The moles of carbon dioxide produced has been:
1 mole propane = 3 moles carbon dioxide
1.5 moles propane = 1.5 [tex]\times[/tex] 3 moles carbon dioxide
1.5 moles propane = 4.5 moles carbon dioxide.
The amount of Carbon dioxide produced with 1.5 moles of propane has been 4.5 moles.
The moles can be expressed as:
Moles = [tex]\rm \dfrac{weight}{molecular\;weight}[/tex]
The molecular weight of carbon dioxide = 44.01 g/mol
The mass of carbon dioxide in 4.5 moles has been:
Mass = Moles [tex]\times[/tex] Molecular weight
Mass of carbon dioxide = 4.5 mol [tex]\times[/tex] 44.01 g/mol
Mass of carbon dioxide = 198.045 grams.
The mass of carbon dioxide produced by burning 1.5 mol of propane has been 198.045 grams.
For more information about the mass-produced, refer to the link:
https://brainly.com/question/6983528
