Question

# 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 productsHence, 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.ScienceNCERTStandard IX

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