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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

Respuesta :

Answer:

Explanation:

a) for 1.000 g X: 0.1621 g Y

ratio of mass of element Y = 2.100g : 0.1621g

= 1 : 0.07

b) 1.000 g X: 0.7391 g Y

ratio of mass of element Y = 2.100g : 0.7391g

= 1: 0.35 , = 20:7

c) 1.000 g X: 0.2579 g Y

ratio of mass of element Y = 2.100g : 0.2579g

= 1 : 0.12

d) 1.000 g X: 0.2376 g Y

ratio of mass of element Y = 2.100g : 0.2376g

= 1: 0.11

e) 1.000 g X: 0.2733 g Y

ratio of mass of element Y = 2.100g : 0.2733g

= 1 : 0.13

From the values obtained , the closest that is in compliance with the law f multiple proportions is option B

Answer:

a. 1.000 g X: 0.1621 g Y.

Explanation:

The law of multiple proportions states that If two elements A and B form more than one compound, then the ratios of the masses of the second element, B which combine with a fixed mass of the first element, A will always be ratios of small whole numbers.

Comparing Compound A; 1.000 g of X : 2.100 with the options given,

a. 0.1621 g of Y : 1.000 g of X

= 2.100 : 0.1621

= 12.96 : 1

= 13 : 1.

b. 0.7391 g of Y : 1.000 g of X

ratio = 2.100 : 0.7391

= 2.84 : 1.

c. 0.2579 of Y : 1.000 g of X

= 2.100 : 0.2579

= 8.143 : 1

d. 0.2376 g of Y : 1000 g of X

= 2.100 : 0.2376

= 8.384 : 1

e. 0.2733 g of Y : 1000 g of X

= 2.100 : 0.2733

= 7.684 : 1

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