QUETION:−
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1.80 g of a certain metal burnt in oxygen gave 3.0 g of its oxide. 1.50 g of the same metal heated in steam gave 2.50 g of its oxide. Show that these results illustrate the law of constant proportion.
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by:- @AngelicCutie
Answers
Answer:
In the first sample of the oxide, <br> wt. of metal=1.80 g, wt. of oxygen =(3.0-1.80)g =1.2 g <br>
<br> In the second sample of the oxide, <br> wt of metal =1.50 g, wt. of oxygen=(2.50-1.50)g =1 g <br>
<br> Thus, in both samples of the oxide the proportions of the weights of the metal and oxygen are fixed. Hence, the results follows the law of constant proportion. <br> Note : This law is not applicable in case of isotopes.
Explanation:
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Answer:
In the first sample of the oxide, <br> wt. of metal=1.80 g, wt. of oxygen =(3.0-1.80)g =1.2 g <br>
<br> In the second sample of the oxide, <br> wt of metal =1.50 g, wt. of oxygen=(2.50-1.50)g =1 g <br>
<br> Thus, in both samples of the oxide the proportions of the weights of the metal and oxygen are fixed. Hence, the results follows the law of constant proportion. <br> Note : This law is not applicable in case of isotopes.
Explanation: