When 3.00 ,g of carbon is burnt in 8.00 ,g of | vedclass

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(A) First,we determine the mass ratio of carbon and oxygen in carbon dioxide $(CO_2)$.The atomic mass of carbon is $12 \,u$ and oxygen is $16 \,u$. In

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$11.00 \,g$ of $CO_2$,Law of Constant Proportions

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(A) First,we determine the mass ratio of carbon and oxygen in carbon dioxide $(CO_2)$.The atomic mass of carbon is $12 \,u$ and oxygen is $16 \,u$. In $CO_2$,the ratio of carbon to oxygen is $12 : (2 	imes 16) = 12 : 32$,which simplifies to $3 : 8$.This means that $3.00 \,g$ of carbon requires exactly $8.00 \,g$ of oxygen to react completely to form $11.00 \,g$ of $CO_2$.When $3.00 \,g$ of carbon is provided with $50.00 \,g$ of oxygen,only $8.00 \,g$ of oxygen will react with the carbon,and the remaining $42.00 \,g$ of oxygen will remain unreacted.Therefore,the mass of $CO_2$ formed remains $11.00 \,g$.This result is governed by the 'Law of Constant Proportions',which states that in a chemical substance,the elements are always present in definite proportions by mass.

When $3.00 \,g$ of carbon is burnt in $8.00 \,g$ of 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?

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