Rebound gpe formula
1 answer:
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Answer:
4.06 mol H₂O
Explanation:
- 2C₆H₁₄ + 19O₂ → 12CO₂ + 14H₂O
First we <em>convert the given masses of reactants into moles</em>, using <em>their respective molar masses</em>:
- 250 g O₂ ÷ 32 g/mol = 7.81 mol O₂
- 50 g C₆H₁₄ ÷ 86 g/mol = 0.58 mol C₆H₁₄
Now we <u>calculate how many O₂ moles would react completely with 0.58 C₆H₁₄ moles</u>, using the <em>stoichiometric coefficients of the reaction</em>:
- 0.58 mol C₆H₁₄ *
= 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 <em>C₆H₁₄ is the limiting reactant</em>.
Now we can <u>calculate how much water can be formed</u>, using <em>the number of moles of the limiting reactant</em>:
- 0.58 mol C₆H₁₄ *
= 4.06 mol H₂O
Answer:
Explanation:
Since we aren't told the mass of material we have, let's assume the boss was generous, and precise, and we have 100.00 grams of the mystery compound. We are told only that hydrogen is 5.988% and that the only other two elements are carbon and oxygen, with equal percentages. (100%-5.988%)/2 = 47.006% of each. See the attached table.
We now have the number of grams of each element, so let's convert that into moles of each by dividing the mass by the element's molar mass, The result in the table is
<u>Moles</u>
C 3.91
H 5.99
O 2.94
We need whole numbers for the empirical formula, so round to C4H6O3, the empirical formula. Possibly acetoacetic acid, a metabolite.
