Questions in chemical-aritmatic

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	The law of multiple proportions is illustrated by the two compounds
	In compound A, 1.00 g nitrogen unites with 0.57 g oxygen. In compound B, 2.00 g nitrogen combines with 2.24 g oxygen. In compound C, 3.00 g nitrogen combines with 5.11 g oxygen. These results obey the following law
	Hydrogen combines with oxygen to form ${H_2}O$ in which 16 g of oxygen combine with 2 g of hydrogen. Hydrogen also combines with carbon to form $C{H_4}$ in which 2 g of hydrogen combine with 6 g of carbon. If carbon and oxygen combine together then they will do show in the ratio of
	2 g of hydrogen combine with 16 g of oxygen to form water and with 6 g of carbon to form methane. In carbon dioxide 12 g of carbon are combined with 32 g of oxygen. These figures illustrate the law of
	An element forms two oxides containing respectively 53.33 and 36.36 percent of oxygen. These figures illustrate the law of
	After a chemical reaction, the total mass of reactants and products
	A sample of pure carbon dioxide, irrespective of its source contains 27.27% carbon and 72.73% oxygen. The data support
	The law of definite proportions is not applicable to nitrogen oxide because
	Which one of the following pairs of compounds illustrates the law of multiple proportion
	Which property of an element is always a whole number