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balanced chemical equation for the decomposition of liquid hydrazine into nitrogen and hydrogen gases with oxygen
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GPT-4o mini
The decomposition of liquid hydrazine (\( \text{N}_2\text{H}_4 \)) into nitrogen (\( \text{N}_2 \)) and hydrogen (\( \text{H}_2 \)) gases in the presence of oxygen (\( \text{O}_2 \)) can be represented by the following balanced chemical equation:
\[
2 \, \text{N}_2\text{H}_4 (l) + 3 \, \text{O}_2 (g) \rightarrow 2 \, \text{N}_2 (g) + 4 \, \text{H}_2 (g) + 2 \, \text{O}_2 (g)
\]
In this equation:
- 2 moles of hydrazine yield 2 moles of nitrogen gas and 4 moles of hydrogen gas, with oxygen being consumed in the reaction.
Please confirm if this interpretation is what you're looking for since the equation presented might suggest different pathways depending on the reaction context.
\[
2 \, \text{N}_2\text{H}_4 (l) + 3 \, \text{O}_2 (g) \rightarrow 2 \, \text{N}_2 (g) + 4 \, \text{H}_2 (g) + 2 \, \text{O}_2 (g)
\]
In this equation:
- 2 moles of hydrazine yield 2 moles of nitrogen gas and 4 moles of hydrogen gas, with oxygen being consumed in the reaction.
Please confirm if this interpretation is what you're looking for since the equation presented might suggest different pathways depending on the reaction context.
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