Two oxides of a certain metal were separately heated in a current of hydrogenuntil constant weights were obtained. The water produced in each case was carefully collected and weighed.2 grams of each oxide gave respectively 0.2517 grams and 0-4526 grams of water. Show that these resultsestablish the Law of Multiple Proportions.
Answers
Answer
these results establish the Law of Multiple Proportions.
Explanation:
Given data:
Two oxides of a certain metal were separately heated in a current of hydrogen.
It was done until constant weights were obtained.
The water produced in each case was carefully collected and weighed
2 grams of each oxide gave respectively 0.2517 grams and 0.4526 grams of water.
To Show that :
these results establish the Law of Multiple Proportions.
Solution:
First we need to calculate the amount of oxygen in each oxide.
For 18 grams of oxygen it is 16 grams of oxygen.
Hence considering the first oxide, that is for
0.2517 grams will require
= 0.2517*16/(18)
= 0.2237 grams oxygen will be required.
Also, 0.4526 water will require
0.4526*16/(18)
=0.4023 grams oxygen will be required
We have to calculate weight of oxygen.
Oxygen combine with 1 g of metal in the given oxide. Weight of given metal oxide is = 2 grams
2-0.2237 = 1.7763 grams will be the required rate of metal. For 2 gram of metal it will be given by
(0.2237/0.7763)* 2.0
= 0.5763 oxygen