When 3.0 g of carbon is burnt in 8.00 g oxygen, 11.00 g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00 g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combinations will govern your answer?
(a) State the postulate of dalton’s atomic theory which can explain the above law.
(b) State the postulate of dalton’s atomic theory which can explain the law of conservation of mass.
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C + O2 → CO2
3 g 8 g 11 g
Total mass of reactants = mass of C + mass of O = 3+8=11g
Total mass of reactants = total mass of products
Hence, the law of conservation of mass is proved.
Further, it also shows carbon dioxide contains carbon and oxygen in a fixed ratio by mass, which is 3 : 8.
Thus it also proves the law of constant proportions. 3 g of carbon must also combine with 8 g of oxygen only. This mean that (50 – 8) = 42 g of oxygen will remain unreacted.
3 g 8 g 11 g
Total mass of reactants = mass of C + mass of O = 3+8=11g
Total mass of reactants = total mass of products
Hence, the law of conservation of mass is proved.
Further, it also shows carbon dioxide contains carbon and oxygen in a fixed ratio by mass, which is 3 : 8.
Thus it also proves the law of constant proportions. 3 g of carbon must also combine with 8 g of oxygen only. This mean that (50 – 8) = 42 g of oxygen will remain unreacted.
dramaqueen4:
thank u
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when 3.00 g of carbon is burnt in 8.00g of oxygen then the mass of carbon dioxide formed =11.00g
according to the law of conservation of mass the total mass before and after the reaction remains same.
3.00g +8.00g =11.00g
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