Question

How many grams of CO2 are produced when 100 g C4H10 undergoes combustion with 200 g O2?

Use the following molar masses: C4H10=58g/mol, O2=32 g/mol and CO2=44g/mol.

Answer 1

2(C₄H₁₀) + 13O₂ → 8CO₂ + 10H₂O

Moles of $C_4H_{10 }= \frac{100}{58}=1.72moles$

Moles of $O_2= \frac{200}{32}=6.25moles$

Moles of $CO_2= \frac{1.72×8}{2}=6.88moles$

Mass of $CO_2= 6.88×44=302.72g$