Answer:
Mass = 299.2 g
Explanation:
Given data;
Mass of butane = 100 g
Mass of oxygen = 350 g
Mass of carbon dioxide produced = ?
Solution:
Chemical equation:
13O₂ + 2C₄H₁₀ → 8CO₂ + 10H₂O
Number of moles of BUTANE:
Number of moles = mass/ molar mass
Number of moles = 100 g / 58.12 g/mol
Number of moles = 1.72 mol
Number of moles of oxygen:
Number of moles = mass/ molar mass
Number of moles = 350 g / 32 g/mol
Number of moles = 11 mol
Now we compare the moles ammonia with hydrogen and nitrogen
O₂ : CO₂
13 : 8
11 : 8/13 ×11 = 6.8 mol
C₄H₁₀ : CO₂
2 : 8
1.72 : 8/2×1.72= 6.88 mol
The number of moles of carbondioxide produced by oxygen are less so it will limiting reactant.
Theoretical yield:
Mass = number of moles × molar mass
Mass =6.8 mol × 44 g/mol
Mass = 299.2 g
