Advertisements
Advertisements
प्रश्न
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 3.00 g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combinations will govern your answer?
Advertisements
उत्तर
| C | + | O2 | → | CO2 |
| 3g | 8g | 11g |
Total mass of reactants = mass of C + mass of O2
= 3 + 8
= 11g
Total mass of reactants = total mass of products
Hence, the law of conservation of mass is proved.
Furthermore, it reveals that carbon dioxide comprises carbon and oxygen in a fixed mass ratio of 3 : 8. Thus, it demonstrates the law of unchanging proportions. 3 g of carbon must combine with only 8 g of oxygen. This means that (50 - 8) = 42 g of oxygen will be unreacted.
APPEARS IN
संबंधित प्रश्न
Which postulate of Dalton’s atomic theory can explain the law of definite proportions?
Name the scientist who gave law of constant proportions.
Name the scientist who gave atomic theory of matter.
The law of constant proportions was given by :
In water, the proportion of oxygen and hydrogen by mass is :
What do we call those particles which have more electrons than the normal atoms ?
What do we call those particles which have less electrons than the normal atoms ?
Work out the formulae for the following compounds :
Sodium oxide
The same proportion of carbon and oxygen in the carbon dioxide obtained from different sources proves the law of ______.
State the law of constant proportions.
