Answer:
Option 1. 0.55 mol of C₄H₁₀
Explanation:
The reaction is:
2C₄H₁₀ + 13O₂ → 8 CO₂ + 10H₂O
This is a combustion reaction where carbon dioxide and water are produced.
We convert mass of produced water to moles → 50 g / 18 g/mol = 2.78 moles of water.
The stoichometry states that:
10 moles of water are made by 2 moles of C₄H₁₀
Therefore 2.78 moles of water will be made by (2.78 . 2) / 10 = 0.55 mol of C₄H₁₀
Answer:
We should use 0.55 moles C4H10 to produce 50 grams of H2O (option 1 is correct)
Explanation:
Step 1: data given
Mass of H2O = 50 grams
Molar mass H2O = 18.02 g/mol
Molar mass C4H10 = 58.12 g/mol
Step 2: The balanced equation
2C4H10 + 13 02 → 8 CO2 + 10H20
Step 3: Calculate moles H2O
Moles H2O = 50.0 grams / 18.02 g/mol
Moles H2O = 2.77 moles
Step 4: Calculate moles C4H10
For 2 moles C4H10 we need 13 moles O2 to produce 8 moles CO2 and 10 moles H2O
For 2.77 moles H2O we need 2.77/5 = 0.55 moles C4H10
We should use 0.55 moles C4H10 to produce 50 grams of H2O (option 1 is correct)
