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 50.00g of oxygen? which law of chemical combination will govern your answer?​

Answer 1

Answer:

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)

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

=3g+8g

=11g

The 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 2

Answer:

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Explanation:

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