更新1:
per the following balanced chemical reaction NH4NO3(s)=N2O(g)+2H2O(g)
how many moles of gas are produced for each 1.00g of NH4NO3?
回答 (1)
2016-05-23 9:36 am
Molar mass of NH₄NO₃ = 14.01×2 + 1.01×4 + 16.00×3 = 80.06 g/mol
Number of moles of NH₄NO₃ used = (1.00 g) / (80.06 g/mol) = 0.0125 mol
NH₄NO₃(s) → N₂O(g) + 2H₂O(g)
According to the equation, the reaction of 1 mole of NH₄NO₃ produces 3 moles of gas (1 mole of N₂O and 2 moles of H₂O).
Number of moles of gas produced = 0.0125 × 3 = 0.0375 mol
Number of moles of NH₄NO₃ used = (1.00 g) / (80.06 g/mol) = 0.0125 mol
NH₄NO₃(s) → N₂O(g) + 2H₂O(g)
According to the equation, the reaction of 1 mole of NH₄NO₃ produces 3 moles of gas (1 mole of N₂O and 2 moles of H₂O).
Number of moles of gas produced = 0.0125 × 3 = 0.0375 mol
收錄日期: 2021-04-18 14:51:45
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20160523005137AAnSfxd