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Accepted Answer
| Question: | 10g Hydrogen (H) + 5g Oxygen (O) |
| Solution: | Water (H₂O) and unreacted Hydrogen |
| Chemical Equation: | 2H₂ + O₂ → 2H₂O |
| Explanation: | The reaction of hydrogen and oxygen is a classic combustion reaction, forming water. However, the provided quantities are not stoichiometrically balanced. 💨 10g of H₂ is approximately 5 moles (10g / 2g/mol). 🧪 5g of O₂ is approximately 0.16 moles (5g / 32g/mol). 🔬 According to the balanced equation, 2 moles of H₂ react with 1 mole of O₂. Therefore, the 0.16 moles of O₂ would only react with 0.32 moles of H₂. This leaves (5 - 0.32 = 4.68) moles of H₂ unreacted. 🔥 The majority of hydrogen will remain unreacted because of the limiting reagent (oxygen) which means that the reaction would primarily form water based on the available oxygen. 💧 |
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