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Compound A and Compound B are binary compounds containing only elements X and Y. Compound A contains 1.000 g of X for every 2.100 g of Y. Which mass ratio for Compound B below follows the law of multiple proportions with Compound A?a. 1.000 g X: 0.1621 g Y b. 1.000 g X: 0.7391 g Y c. 1.000 g X: 0.2579 g Y d. 1.000 g X: 0.2376 g Y e. 1.000 g X: 0.2733 g Y

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IthaloAbreu

Answer:

a

Explanation:

The Law of Multiple Proportions is the third postulate of Dalton, and it stated that in a compound, the mass of one element combines with a fixed mass of the other element in a proportional ratio of whole numbers.

In the compound A, the mass of Y per gram of X is 2.100 g of Y per g of X. Thus, let's analyze the letters, and identify in which the ratio will be a whole number:

a. 0.1621 g of Y per g of X

ratio = 2.100 : 0.1621 (Dividing both for 0.1621)

ratio = 12.9 : 1

Which ca be approximate to 13 : 1, a whole number

b. 0.7391 g of Y per g of X

ratio = 2.100 : 0.7391 (Diving both for 0.7391)

ratio = 2.84 : 1

Which is not a whole number

c. 0.2579 of Y per g of X

ratio = 2.100 : 0.2579 (Dividing both for 0.2579)

ratio = 8.143 : 1

Which is not a whole number

d. 0.2376 g of Y per g of X

ratio = 2.100 : 0.2376 (Dividing both for 0.2376)

ratio = 8.384 : 1

Which is not a whole number

e. 0.2733 g of Y per g of X

ratio = 2.100 : 0.2733 (Dividing both for 0.2733)

ratio = 7.684 : 1

Which is not a whole number

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