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?
Answers
Answer:
answer is 50 g +3g
=53g
so, 53g co2 is formed.
this shows law of conservation of mass.
hope it helps you
Answer:
Explanation:
Carbon and oxygen react to form carbon dioxide according to the equation Carbon (C) + Oxygen (O2) > Carbon dioxide (CO2)
In the first case :
3.0 g of carbon are burnt in 8.0 g of oxygen to form 11.0 g of CO2 In the second case :
3.0 g of carbon must also combine with 8.0 g of oxygen only. This means that (50 – 8) = 42 g of oxygen will remain unreacted.
The mass of CO2 in this case must be also 11 g.
The answer is based on Law of constant proportions.
In the second case, only 8.0 g of oxygen react although 50.0 g are available. This shows that the mass of carbon dioxide (11.0 g) formed depends upon the mass of carbon (3.0 g) or the substance present in smaller amount. In general, the substance (element or compound) present in smaller amount in a reaction limits the participation of the other reactants. It is quite often called limiting reactant. Carbon is the limiting reactant in this case. It limits the participation of oxygen and also the formation of carbon dioxide.