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?

Explanation

`underset(3 g)( C) + underset(8 g)(O_(2)) to underset(11 g)(CO_(2))`
Total mass of reactants = mass of C + mass of `O_(2) = 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 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.