Question

2 C6H14 + 19 O2 --> 12 CO2 + 14 H2O

Answer 1

Answer:

4.06 mol H₂O

Explanation:

• 2C₆H₁₄ + 19O₂ → 12CO₂ + 14H₂O

First we convert the given masses of reactants into moles, using their respective molar masses:

• 250 g O₂ ÷ 32 g/mol = 7.81 mol O₂

• 50 g C₆H₁₄ ÷ 86 g/mol = 0.58 mol C₆H₁₄

Now we calculate how many O₂ moles would react completely with 0.58 C₆H₁₄ moles, using the stoichiometric coefficients of the reaction:

• 0.58 mol C₆H₁₄ * $\frac{19molO_2}{2molC_6H_{14}}$ = 5.51 mol O₂

As there are more O₂ moles than required (7.81 vs 5.51), O₂ is the reactant in excess. That means that C₆H₁₄ is the limiting reactant.

Now we can calculate how much water can be formed, using the number of moles of the limiting reactant:

• 0.58 mol C₆H₁₄ * $\frac{14molH_2O}{2molC_6H_{14}}$ = 4.06 mol H₂O