Answer:
Explanation:
Given data:
Mass of octane = 55.5 g
Balanced chemical equation = ?
Mass of oxygen required to react = ?
Mass of CO₂ for med = ?
Molecules of water produced = ?
Mass of octane required to produced 30.0 g of water = ?
Solution:
1)
Chemical equation:
2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O
2)
Mass of oxygen required to react = ?
Mass of octane = 55.0 g
Solution:
Number of moles of octane:
Number of moles = mass/ molar mass
Number of moles = 55.0 g/114.23 g/mol
Number of moles = 0.48 mol
Now we will compare the moles of octane with oxygen.
C₈H₁₈ : O₂
2 : 25
0.48 : 25/2×0.48 = 6 mol
Mass of oxygen required:
Mass = number of moles × molar mass
Mass = 6 mol × 32 g/mol
Mass = 192 g
3)
Given data:
Mass of carbon dioxide produced = ?
Mass of octane = 55g
Solution:
Number of moles of octane:
Number of moles = mass/ molar mass
Number of moles = 55.0 g/114.23 g/mol
Number of moles = 0.48 mol
Now we will compare the moles of octane with CO₂.
C₈H₁₈ : CO₂
2 : 16
0.48 : 16/2×0.48 = 3.84 mol
Mass of CO₂ produced:
Mass = number of moles × molar mass
Mass = 3.84 mol × 44 g/mol
Mass = 168.96 g
4)
Given data:
Molecules of water produced = ?
Mass of octane = 55g
Solution:
Number of moles of octane:
Number of moles = mass/ molar mass
Number of moles = 55.0 g/114.23 g/mol
Number of moles = 0.48 mol
Now we will compare the moles of octane with H₂O.
C₈H₁₈ : H₂O
2 : 18
0.48 : 18/2×0.48 = 4.32 mol
Number of molecules of water:
1 mol = 6.022× 10²³ molecules
4.32 mol × 6.022× 10²³ molecules/ 1 mol
26 × 10²³ molecules
5)
Given data:
Mass of octane required = ?
Mass of water produced = 30 g
Solution:
Number of moles of water.
Number of moles = mass/ molar mass
Number of moles = 30 g/ 18 gmol
Number of moles = 1.67 mol
Now we will compare the moles of water and octane from balance chemical equation:
2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O
H₂O : C₈H₁₈
18 : 2
1.67 : 2/18×1.67 = 0.185 mol
Mass of octane:
Mass = number of moles ×molar mass
Mass = 0.185 × 114.23 g/mol
Mass = 21.13 g
