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₮m³== Examples Of Laws Of Chemical Combinations == Example1::2.34 g of carbon reacts with oxygen to give 5.46 g of one oxide while 1.8 g of carbon reacts with oxygen to give 6.6 g of another oxide. Show that the observeation confirms the law of multiple proportions. Solution:           I : Mass of C = 2.34 g                             Mass of O = 5.46-2.34 = 3.12g ⇒ 1 g of C reacts with 3.12/2.34 g of O to give oxide I                         II :    Mass of C = 1.8 g                                  Mass of O = 6.6-1.8 = 4.8 g                        ⇒ 1 g of C reacts with 4.8/1.8 g of O to give oxide II                         The ratio of masses of oxygen required to react with 1 g of carbon is                                                3.12/2.34 : 4.8/1.8 = 1:2                        Hence, the law is proved. ---                    == Do It Your Self==

Example
1: Which Law of chemical combinations can be verified from the given data? Analysis of pure CaCO3 collected from different sources has: Source I: Ca=12 mg,C=3.6 mg ,O=14.4 mg                       Source II: Ca= 15.6 mg,C = 4.68 mg,O = 18.72 mg

Example
2:If 1.2 m³ of oxygen at a certain temperature and pressure has x molecules , then what is the number of molecules present in 3 m³ of CO2 maintained at same temperature and pressure?