when 3.0 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 ?
Answers
First, let us write the reaction taking place here
C + O2 → CO2
As per the given condition, when 3.0 g of carbon is burnt in 8.00 g oxygen, 11.00 g of carbon dioxide is produced.
3g + 8g →11 g ( from the above reaction)
Total mass of reactants = mass of carbon + mass of oxygen
=3g+8g
=11g
Total mass of reactants = Total mass of products
Therefore, the law of conservation of mass is proved.
Then, it also depicts that the carbon dioxide contains carbon and oxygen in a fixed ratio by mass, which is 3:8.
Thus it further proves the law of constant proportions.
3 g of carbon must also combine with 8 g of oxygen only.
This means that (50−8)=42g of oxygen will remain unreacted.
The remaining 42 g of oxygen will be left un-reactive. In this case also, only 11 g of carbon dioxide will be formed
The above answer is governed by the law of constant proportions.
Answer:
As per the given condition, when 3.0 g of carbon is burnt in 8.00 g oxygen, 11.00 g of carbon dioxide is produced. Therefore, the law of conservation of mass is proved. Then, it also depicts that the carbon dioxide contains carbon and oxygen in a fixed ratio by mass, which is 3:8.