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The following table gives observations on two gaseous reaction. In each set, the temperature and pressure conditions are kept fixed.A.Nitrogen gasHydrogen gas (cm)3Ammonia gas (cm)3623.3349.084.71830.01051.2251.91253.4685.6170.7B.Hydrogen gas(cm)3Oxygen gas (cm)3Water vapour (cm)3307.9435.9851.1156.6217.8473.1309.1432.6856.0What do you infer from this data? Can you understand the law you have inferred empirically on the basis of the atomic picture and Avogadro's hypothesis? |
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Answer» In part A, ratio of volume of hydrogen gas to that of nitrogen is nearly equal to 3 (actually in each of the three cases, the ratio is 2.94, 3.01 and 2.97. respectively). It indicates that the three molecules of hydrogen combine with one molecule of nitrogen to form one molecule of ammonia gas. In part B, the ratio of the volume of hydrogen to that of oxygen is about 2 (actually in three cases, the ratio is 1.97, 2.00, 1.8 respectively. It indicates that two molecules of hydrogen combine with one molecule of oxygen to form one molecule of water. From above, we find that the two gases combine chemically to yield another gas at the same temperature and pressure and the volumes of these gases bear simple ratio of small integers. This is the Gay Lussac's law. We can also understand the law on the basis of atomic picture and Avogadro's hypothesis. |
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