The discussion confirms that the reaction of 50 cm³ of nitrogen gas combining with 150 cm³ of hydrogen gas to produce 100 cm³ of ammonia adheres to Gay-Lussac's Law of combining volumes. According to the law, the ratio of gas volumes corresponds to the ratio of their respective molecules. The reaction can be represented as N2 + 3H2 → 2NH3, which supports the volume ratio of 1:3:2, validating the conclusion that the resulting 100 cm³ of ammonia is consistent with the law.
PREREQUISITESChemistry students, educators, and professionals interested in gas behavior and chemical reactions will benefit from this discussion, particularly those focusing on stoichiometry and gas laws.
markosheehan said:50 cm^3 of nitrogen combine with 150 cm^3 of hydrogen gas to form 100 cm^3 of ammonia. Does this agree with gay lussacs law of combing volumes?. Explain your answer.
i feel the answer is yes but I can not give the reason why?
thank you very muchI like Serena said:The reaction is:
$$\ce{N2 + 3H2 \to 2NH3}$$
Gay-Lussac says that the ratio of molecules corresponds to the ratio of volumes of gasses.
That is:
$$1:3:2 = 50 \text{ cm}^3 : 150 \text{ cm}^3 : 100 \text{ cm}^3$$
Therefore the $100 \text{ cm}^3$ of ammonia does indeed agree with Gay-Lussac's law.