Question
c2h6 3o2 2co2 3h2o
Answers
GPT-4o mini
The chemical equation you've provided appears to represent the combustion of ethane (C₂H₆) in the presence of oxygen (O₂), producing carbon dioxide (CO₂) and water (H₂O). The balanced equation for this combustion reaction is:
\[
2 \, \text{C}_2\text{H}_6 + 7 \, \text{O}_2 \rightarrow 4 \, \text{CO}_2 + 6 \, \text{H}_2\text{O}
\]
Here's a breakdown of the process:
1. **Reactants:**
- Ethane (\(C_2H_6\)) - a hydrocarbon.
- Oxygen (\(O_2\)) - required for combustion.
2. **Products:**
- Carbon dioxide (\(CO_2\)) - produced from the carbon in the ethane.
- Water (\(H_2O\)) - produced from the hydrogen in the ethane.
To balance the equation:
- For every 2 moles of ethane, you need 7 moles of oxygen to fully combust it, producing 4 moles of carbon dioxide and 6 moles of water.
If you have any specific questions or need further clarification about this reaction, feel free to ask!
\[
2 \, \text{C}_2\text{H}_6 + 7 \, \text{O}_2 \rightarrow 4 \, \text{CO}_2 + 6 \, \text{H}_2\text{O}
\]
Here's a breakdown of the process:
1. **Reactants:**
- Ethane (\(C_2H_6\)) - a hydrocarbon.
- Oxygen (\(O_2\)) - required for combustion.
2. **Products:**
- Carbon dioxide (\(CO_2\)) - produced from the carbon in the ethane.
- Water (\(H_2O\)) - produced from the hydrogen in the ethane.
To balance the equation:
- For every 2 moles of ethane, you need 7 moles of oxygen to fully combust it, producing 4 moles of carbon dioxide and 6 moles of water.
If you have any specific questions or need further clarification about this reaction, feel free to ask!