Moles of ammonia
- Given mass/Molar mass
- 230/17
- 13.5mol
1mol requires 5.66KJ energy
13.5mol requires
Answer:
Explanation:
1. Calculate the mass of each reactant gas in the mixture
<u>a) CH₄</u>
- 28.6% of 289g
- 0.286 × 289g = 82.654g
<u>b) C₃H₈</u>
- 71.4% of 289g
- 0.714 289g = 206.346g
2. Calculate the mass of CO₂ produced by each gas in the mixture
<u>a) CH₄</u>
i) Balanced chemical equation:
- CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g)
ii) Number of moles of CH₄:
- number of moles = mass in grams / molar mass
- molar mass of CH₄ = 16.04g/mol
- number of moles = 82.654g / 16.04 g/mol = 5.153 mol
iii) Number of moles of CO₂
- From the balanced chemical equation, the mole ratio is 1 mol CH₄ : 1 mol CO₂.
- Hence, 5.153 mol of CO₂ are produced
iv) Convert the number of moles to mass
- mass = number of moles × molar mass
- molar mass of CO₂ = 44.01g/mol
- mass = 5.153 mol × 44.01g/mol = 226.8 g
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<u>b) C₃H₈</u>
i) Balanced chemical equation:
- C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(g)
ii) Number of moles of C₃H₈:
- number of moles = mass in grams / molar mass
- molar mass of C₃H₈ = 44.1g/mol
- number of moles = 206.346g / 44.1 g/mol = 4.679 mol
iii) Number of moles of CO₂
- From the balanced chemical equation, the mole ratio is 1 mol C₃H₈ : 1 mol CO₂.
- Hence, 4.679 mol of CO₂ are produced
iv) Convert the number of moles to mass
- mass = number of moles × molar mass
- molar mass of CO₂ = 44.01g/mol
- mass = 4.679 mol × 44.01g/mol = 205.9 g
3. Total mass of CO₂
Add the two values found above:
Round to 3 significant figures: 433g.
The answer is C because The products are way more stable than the reactants.
