Two samples of carbon tetrachloride are decomposed into their constituent elemen

Question

Two samples of carbon tetrachloride are decomposed into their constituent elements. One sample produces 38.8 g of carbon and 447 g of chlorine, and the other sample pro 19.4 g of carbon and 176 g of chlorine. Are these results consistent with the law of definite proportions? Explain your answer. Results are consistent with the law of definite proportions because the ratio of the mass of chlorine from one compound to the mass of chlorine in the other is a small whole number. Results are not consistent with the law definite proportions because the mass ratios of chlorine to carbon both samples are not small whole numbers. Results are consistent with the law of definite proportions because the mass ratios of chlorine to both samples are the same. Results are not with the law of definite proportions because the mass ratios of chlorine to carbon for both sample are not the same.

Explanation / Answer

the law of definite proportions, states that a given chemical compound always contains its component elements in fixed ratio (by mass) and is independent of its source.

Accordingly CCl4----->C + 2Cl2

mass of C produced = 38.8 gm and mass of Cl2 = 447 gm

moles of C=38.8/12 =3.23 and moles of Cl2 = 447/71=6.295, mole Ratio of Cl2: C = 6.295/3.23= 1.94

for the second case, moles of C = 19.4/12 =1.62 and Cl2 = 176/71= 2.48 , moles ratio = 2.48/1.62=1.53

The ratio is different and hence is not as per law of definite proportions. D is correct.

for the second case, mass of C= 19.4 gm and mass of Chlorine

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