Question

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 3.0 g of carbon is burnt in 50.00 g of oxygen which law of chemical combination will govern your answer​

Answer 1

Explanation:

Given that

3.0 g of carbon combines with 8.0 g of oxygen to give 11.0 of carbon dioxide.

Find out

We need to find out the mass of carbon dioxide will be formed when 3.00 g of carbon is burnt in 50.00 g of oxygen.

Solution

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 2

Answer:

11g of $CO_2$

Explanation:

$C + O_2 --> CO_2$

3g + 8g - -> 11 g

given mass of Carbon (C) = 3g

given mass of Oxygen ($O_2$) = 50g

∴ Carbon will be the limiting Reagent and Oxygen will be the excess reagent.

∴ 11g of  Carbon dioxide will be formed with 42 g of excess $O_2$