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When $$3.0\ g$$ of carbon is burnt in $$8.00\ g$$ oxygen, $$11.00\ g$$ of carbon dioxide is produced? What mass of carbon dioxide will be formed when $$3.00\ g$$ of carbon is burnt in $$50.00\ g$$ of oxygen? Which law of chemical combination will govern your answer?


Solution

$$C + O_2\rightarrow CO_2$$
$$3 g$$    $$8 g$$         $$11 g$$
Total mass of reactants = mass of carbon + mass of oxygen $$= 3 +8 =11 g$$
Total mass of reactants = Total mass of products

Hence, the law of conservation of mass is proved.

Further, it also shows carbon dioxide contains carbon and oxygen in a fixed ratio by mass, which is 3:8.

Thus it also proves the $$\text {law of constant proportions}$$. 3 g of carbon must also combine with 8 g of oxygen only.
This means that $$(50-8)=42 g$$ of oxygen will remain unreacted.

Science
NCERT
Standard IX

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