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 3.00g the of carbon is burnt in 50.00g of oxygen? which law of chemical Combination Will Govern Your answer​

Answer 1

Answer

11 g, law of constant proportions

Explanation

When 3 g of Carbon is burnt with 8 g of oxygen, 11 g of carbon dioxide is produced.

$\sf C + O_2 \rightarrow CO_2$

If, 3 g of carbon is burnt in 50 g of oxygen, then also only 8 g of oxygen would take part in reaction and the remaining 42 g of oxygen would be unaffected. This is because the 3 g of carbon acts as a limiting reagent for the reaction. Hence, 11 g of carbon dioxide will be formed.

The law of constant proportion (the compound is present in its fixed ratio, not depending on the source or method from where it is obtained) is responsible for the reason.

Answer 2

Answer:

$\large\boxed{\sf{11.00 \:g}}$

$\large\boxed{\sf{Law\:Of\: Constant\: Proportion}}$

Explanation:

Given that, when 3.0 g of carbon is burnt in 8.0 g of oxygen, 11.0 g of carbon dioxide is formed.

The reaction involved in this process is :$\;\;\;\;\;\;\;\;\;\;\large{\sf{C+O_{2}\rightarrow CO_{2}}}$

• Now, when 3.0 g of carbon is burnt in 50.0 g of oxygen, only 8.0 g of oxygen will take part in the reaction.
• The rest 42.0 g will be left unreacted.
• This is due to the Carbon acting as limiting reagent.
• This means that no carbon will be left after reaction of 8.0 g of oxygen.
• That's why, 42.0 g of oxygen will be left unreacted.

Hence, again 11.0 g of carbon dioxide will be formed.

This answer is governed by the LAW OF CONSTANT PROPORTION.