Commonly Searched Equations
Questions asked by users might not always be phrased in the clearest way.
Accepted Answer
| Question: | 10g Hydrogen (H) + 10g Oxygen (O) |
| Solution: | Approximately 11.25g of water (H₂O) and 8.75g of unreacted oxygen (O₂) |
| Chemical Equation: | 2H₂ + O₂ → 2H₂O |
| Explanation: | We start with 10g of Hydrogen (H₂) and 10g of Oxygen (O₂). 🤔 First, we convert the masses to moles using their molar masses: H₂ (2 g/mol) and O₂ (32 g/mol). This gives us 5 moles of H₂ and 0.3125 moles of O₂. According to the balanced equation, 2 moles of H₂ react with 1 mole of O₂. ✨ We have excess Hydrogen. The 0.3125 moles of O₂ will react with 0.625 moles of H₂ producing 0.625 moles of H₂O. Converting this back to grams using the molar mass of water (18 g/mol), we get approximately 11.25g of water. The remaining Hydrogen does not react. 🧪 The remaining oxygen is 10g - (0.625 moles H₂ * 32 g/mol O₂ /2 moles H₂) ≈ 8.75g of O₂ |
Looking for something different?
Join our free Chemistry AI platform and create your own experiments.
