How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 42.1 moles of water vapor?
2 answers:
Answer: 84.2 mol hydrogen gas (H₂) woiuld be needed to react with excess carbon dioxide to produce 42.1 moles of water vapor.
Explanation:
1) <u>Word equation</u>:
hydrogen (g) + carbon dioxide (g) → water (g) + methane (g)
2) <u>Molecular equation</u>:
H₂(g) + CO₂(g)→ H₂O(g) + CH₄(g)
3) <u>Balanced molecular equation</u>:
4H₂(g) + CO₂(g)→ 2H₂O(g) + CH₄ (g)
4) <u>Stoichiometric mole ratios</u>:
4 mol H₂ : 1 mol CO₂ : 2 mol H₂O(g) : 1 mol CH₄
5) <u>Set a proportion with the stoichiometric mole ratios, the moles of water vapor produced and the unknown:</u>
4 mol H₂ / 2 mol H₂O = x / 42.1 mol H₂O ⇒ x = 42.1 mol H₂O × 4 mol H₂ / 2 mol H₂O = 84.2 mol H₂ ← answer
Answer:
84.2 moles of hydrogen gas will be needed to produce 42.1 moles of water vapors.
Explanation:
According to reaction 4 moles of hydrogen gas gives 2 moles of water vapor.
Then, 42.1 moles of water vapor will be produced by:
hydrogen gas
84.2 moles of hydrogen gas will be needed to produce 42.1 moles of water vapors.
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