Advertisements
Advertisements
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 3.00 g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combinations will govern your answer?
Advertisements
Solution
| 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
RELATED QUESTIONS
Name the scientist who gave law of constant proportions.
Which part of the Dalton's atomic theory came from the law of constant proportions given by Proust ?
Name any two laws of chemical combination.
Give one major drawback of Dalton's atomic theory of matter.
Which postulate of Dalton’s atomic theory can explain the law of constant proportions ?
When 5 g of calcium is burnt in 2 g of oxygen, then 7 g of calcium oxide is produced. What mass of calcium oxide will be produced when 5 g of calcium is burnt in 20 g of oxygen ? Which law of chemical combination will govern your answer ?
What do we call those particles which are formed by the loss of electrons by atoms ?
Work out the formulae for the following compounds :
Sodium oxide
Work out the formulae for the following compounds:
Calcium carbonate
State the law of constant proportions.
