Answer :
Answer
448.902 grams CO2
Explanation
Given:
The mass of propane lost = 150.0 g
What to find:
The grams of carbon dioxide produced.
Step-by-step solution:
The first step is to write a balanced chemical equation for the reaction.
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
The next step is to convert 150.0 g C3H8 to moles using the mole formula
[tex]Mole=\frac{Mass}{Molar\text{ }mass}[/tex]The molar mass of C3H8 = 44.1 g/mol
[tex]Mole=\frac{150.0\text{ }g}{44.1\text{ }g\text{/}mol}=3.40\text{ }mol\text{ }C_3H_8[/tex]Now, use the mole ratio in the equation and the mole of propane lost to calculate the mole of carbon dioxide produced.
From the equation;
1 mole of C₃H₈ produces 3 moles of CO₂
Therefore, 3.40 moles of C₃H₈ will produce
[tex]\frac{3.40\text{ }mol\text{ }C_3H_8}{1\text{ }mol\text{ }C_3H_8}\times3\text{ }mol\text{ }CO_2=10.2\text{ }mol\text{ }CO_2[/tex]The final step is to convert 10.2 moles of CO2 produced to grams using the mole formula in step 2 above.
Molar mass of CO2 = 44.01 g/mol
[tex]\begin{gathered} Mole=\frac{Mass}{Molar\text{ }mass} \\ \\ \Rightarrow Mass=Mole\times Molar\text{ }mass=10.2mol\times \\ \\ Mass=10.2\text{ }mol\times44.01g\text{/}mol=448.902\text{ }grams \end{gathered}[/tex]Therefore, the grams of carbon dioxide produced is 448.902 grams