Compound A and Compound B are binary compounds containing only elements X and Y. Compound A contains 1.000 g of X for every 2.10

For 1.000 g of X, the mass of Y is 0.1621 g. The mass ratio of Y = 2.100 g: 0.1621 g equals 1:0.07. For 1.000 g of X, the mass of Y is 0.7391 g, which leads to a mass ratio of Y = 2.100 g: 0.7391 g simplifying to 1:0.35 or 20:7. For 1.000 g of X, the corresponding mass of Y is 0.2579 g, yielding a mass ratio of Y = 2.100 g: 0.2579 g resulting in 1:0.12. For 1.000 g of X, the mass of Y becomes 0.2376 g, giving a mass ratio of Y = 2.100 g: 0.2376 g, simplifying to 1:0.11. Lastly, for 1.000 g of X, the mass of Y is determined to be 0.2733 g, leading to a mass ratio of Y = 2.100 g: 0.2733 g which reduces to 1:0.13. Among the calculated values, option B aligns most closely with the law of multiple proportions.

The answer is a) 1.000 g of X: 0.1621 g of Y. The law of multiple proportions dictates that if two elements, A and B, create more than one compound, the ratios of the masses of B that combine with a fixed mass of A will always yield small whole number ratios. Analyzing Compound A; 1.000 g of X is to 2.100 g. Comparing it with the options: a) 0.1621 g of Y to 1.000 g of X results in 2.100:0.1621, which simplifies to 12.96:1, approximating to 13:1. b) Y being 0.7391 g to 1.000 g leads to a mass ratio of 2.100:0.7391, resolving to 2.84:1. c) With Y being 0.2579 g to 1.000 g, the ratio yields 2.100:0.2579, which is 8.143:1. d) For 0.2376 g of Y to 1.000 g of X, it results in 2.100:0.2376, or 8.384:1. e) 0.2733 g of Y to 1.000 g produces 2.100:0.2733, which gives 7.684:1.