An element forms two oxides of 2.9 g and 2.25 g of these oxides each was found to contain 1.12 L of O2 at STP. What is the simple ratio if it obeys law of multiple proportions?
An element forms two oxides of 2.9 g and 2.25 g of these oxides each was found to contain 1.12 L of O2 at STP. What is the simple ratio if it obeys law of multiple proportions?
The correct option is B 2:1
According to gram molecular volume law, 22.4 L of all gases at STP weigh equal to their molecular weights denoted in grams. Hence, the weight of 1.12 L of oxygen at STP
= 32×1.1222.4 = 1.6g
In the first oxide:
Weight of oxide = 2.9 g; weight of O = 1.6 g
∴ Weight of the element = 2.9 - 1.6 = 1.300 g
In the other oxide:
Weight of oxide = 2.250 g; weight of O = 1.600 g
Weight of element = 2.25- 1.6 = 0.650 g
Thus, the weights of the element that combine with the same weight of oxygen in its two oxides are in the ratio of 1.3 : 0.65 or 2 : 1 a simple ratio. Hence, it illustrates the law of multiple proportions.
2:1
According to gram molecular volume law, 22.4 L of all gases at STP weigh equal to their molecular weights denoted in grams. Hence, the weight of 1.12 L of oxygen at STP
= 32×1.1222.4 = 1.6g
In the first oxide:
Weight of oxide = 2.9 g; weight of O = 1.6 g
∴ Weight of the element = 2.9 - 1.6 = 1.300 g
In the other oxide:
Weight of oxide = 2.250 g; weight of O = 1.600 g
Weight of element = 2.25- 1.6 = 0.650 g
Thus, the weights of the element that combine with the same weight of oxygen in its two oxides are in the ratio of 1.3 : 0.65 or 2 : 1 a simple ratio. Hence, it illustrates the law of multiple proportions.
