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標題:
CHEM 計mole 既數
發問:
When sodium is heated in air, it catches fire and forms an oxide. If the sample is weighed before and after reaction, it is found to increase in mass by approximately 35%. On the other hand , when sodium is heated in pure oxygen, the reaction takes place more readily and the increase in mass is about 70%. Work out... 顯示更多 When sodium is heated in air, it catches fire and forms an oxide. If the sample is weighed before and after reaction, it is found to increase in mass by approximately 35%. On the other hand , when sodium is heated in pure oxygen, the reaction takes place more readily and the increase in mass is about 70%. Work out the empirical formulae of the two oxides of sodium. 唔識計唔該幫幫手!! 唔該要有steps!!! 唔該晒(:
Consider the first oxide. Mole ratio Na : O = 100/23 : 35/16 = 4.35 : 2.19 ≈ 2 : 1 Empirical formula of the first oxide = Na2O Consider the second oxide. Mole ratio Na : O = 100/23 : 70/16 = 4.35 : 4.38 ≈ 1 : 1 Empirical formula of the second oxide = NaO
其他解答:
CHEM 計mole 既數
發問:
When sodium is heated in air, it catches fire and forms an oxide. If the sample is weighed before and after reaction, it is found to increase in mass by approximately 35%. On the other hand , when sodium is heated in pure oxygen, the reaction takes place more readily and the increase in mass is about 70%. Work out... 顯示更多 When sodium is heated in air, it catches fire and forms an oxide. If the sample is weighed before and after reaction, it is found to increase in mass by approximately 35%. On the other hand , when sodium is heated in pure oxygen, the reaction takes place more readily and the increase in mass is about 70%. Work out the empirical formulae of the two oxides of sodium. 唔識計唔該幫幫手!! 唔該要有steps!!! 唔該晒(:
- f3 mth questions!!!急~聽日要交!@1@
- 急(星期三前要啦~)~麻煩幫幫忙~
- please.................................help!!!!!!!!!!!!!!!!!@1@
- f3 mth questions!!!急~聽日要交!@1@
- 急(星期三前要啦~)~麻煩幫幫忙~
- please.................................help!!!!!!!!!!!!!!!!!@1@
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最佳解答:Consider the first oxide. Mole ratio Na : O = 100/23 : 35/16 = 4.35 : 2.19 ≈ 2 : 1 Empirical formula of the first oxide = Na2O Consider the second oxide. Mole ratio Na : O = 100/23 : 70/16 = 4.35 : 4.38 ≈ 1 : 1 Empirical formula of the second oxide = NaO
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