Question

. 3 g of carbon on burning in 8 g oxygen produces 11 g of carbon dioxide. What mass of carbon dioxide will be formed when 3 g of carbon is burnt in 50 g of oxygen? which law of chemical combination will govern your answer?


Ishu (ishu995)please answer this also
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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

$\huge\pink{\underline{Question:}}$

When 3 g of carbon on burning in 8 g oxygen produces 11 g of carbon dioxide. What mass of carbon dioxide will be formed when 3 g of carbon is burnt in 50 g of oxygen? which law of chemical combination will govern your answer?

$\huge\green{\underline{Answer:}}$

Our answer will be governed by the law of constant proportions.

Now, since carbon and oxygen combine in the fixed proportion of 3 : 8 by the mass to produce 11 g of carbon dioxide, therefore, the mass of carbon dioxide (11 g) will be obtained even if we burn 3 g of carbon in50 g of oxygen.

The extra oxygen (50 - 8 = 42 g oxygen) will remain unreacted.

$\huge\purple{\underline{Hope \: it \: is \: helpful}}$