Question

2. 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 3.00g of carbon is burnt in 50.00 g of oxygen? which law of chemical combination will govern your answer?​

Answer 1

Answer:

1.5 carbon dioxide are realse from him

Answer 2

Answer for the following question :-

When 3.0 g of carbon is burnt in 8.00 g of oxygen, 11.00 g of carbon dioxide is produced.

3g carbon + 8g oxygen = 11g Carbon dioxide

Thus,

The ratio in which carbon and oxygen combine to give carbon dioxide is 3:8.

Now,

GIVEN :-

Mass of carbon = 3.00 g

Mass of oxygen = 50.00 g

TO FIND :-

Mass of carbon dioxide formed = ?

SOLUTION :-

When 3g of carbon is burnt in 50g of oxygen,

only 8g of oxygen will be used to burn 3g of carbon to provide carbon dioxide as the ratio to form carbon dioxide is 3:8.

The total mass of reactants = mass of carbon + mass of oxygen

=3g+8g

=11g

Here,

Carbon dioxide contains carbon and oxygen in a fixed ratio by mass, which is 3:8.

This proves the law of constant proportions.

So,

3g of carbon must react only with 8g of oxygen to form 11g of carbon dioxide.

The leftover oxygen will remain unreacted.

= (50g - 8g) oxygen

= 42g oxygen

FINAL ANSWER :-

MASS OF CARBON DIOXIDE FORMED IS 11g FOR 3g CARBON AND 50g OXYGEN.

THIS ANSWER IS GOVERNED BY THE CHEMICAL COMBINATION LAW OF CONSTANT PROPORTION GIVEN BY JOSEPH PROUST.