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Accepted Answer
| Question: | 100g Hydrogen (H) + 100g Oxygen (O) |
| Solution: | Approximately 112.5g of water (H₂O) and 87.5g of unreacted Oxygen (O₂) |
| Chemical Equation: | 2H₂ + O₂ → 2H₂O |
| Explanation: | The reaction between hydrogen and oxygen follows the stoichiometry indicated in the balanced chemical equation. First, we convert the masses to moles: 100g H₂ is approximately 50 moles (100g / 2g/mol) and 100g O₂ is approximately 3.125 moles (100g / 32g/mol). 🤔 According to the equation, 2 moles of H₂ react with 1 mole of O₂. Therefore, 50 moles of H₂ would require 25 moles of O₂. 💥Since we only have 3.125 moles of O₂, oxygen is the limiting reactant. 🧪 The amount of water produced is determined by the amount of limiting reactant: 3.125 moles O₂ will produce 6.25 moles H₂O. Converting back to grams, 6.25 moles H₂O * 18 g/mol ≈ 112.5g H₂O. 🎉 The remaining oxygen is 100g - (3.125moles * 32g/mol) = 87.5g. |
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