2.0 g of a metal burnt in oxygen gave 3.2 g of its oxide. 1.42 g of the same metal heated in steam gave 2.27 of its oxide. Which law is verified by these data?
Answers
Answer:
Step-by-step explanation:
In the first sample of the oxide, wt. of metal = 2.0g
wt. of oxygen = (3.2 - 2)g
= 1.2g
=> wt. of metal / wt. of oxygen
= 2.0g / 1.2g = 1.67
In the second sample of the oxide, wt. of metal = 1.42g
wt. of oxgen = (2.27 - 1.42)g
= 0.85g
=> wt. of metal / wt. of oxygen
= 1.42g / 0.85
= 1.67
Thus in both smaples of the oxide the proportions of the weights of the metal and oxgen are fixed. Hence, the results follows the law of constant proportion.
Note: This law is not applicable in isotopes .
Answer:
Step-by-step explanation:
When two gms of metal burns with oxygen, it gives 3.2 gms of its oxide.
Thus,
Ratio of M:O = 2/3.2
Ratio of M:O = 0.625
When 1.42 gms of metal is heated with steam, it gives 2.27 gms of its oxide.
Ratio of M:O = 1.42/2.27
Ratio of M:O = 0.625
Hence, the ratio of metal to oxygen in its oxide is the same (0.625) irrespective of its method of preparation.
This is called the law of definite proportions. The law states that a given chemical compound will always contain its component elements in a fixed ratio and it does not depend on its source and the method of preparation.