When 3.0g of carbon is burnt in 8.00g oxygen, 11.00g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00g of carbon is burnt in 50.0g of oxygen? Which law of chemical combination will govern your answer?
When 3.0g of carbon is burnt in 8.00g oxygen, 11.00g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00g of carbon is burnt in 50.0g of oxygen? Which law of chemical combination will govern your answer?
Solution and Explanation
First we find the proportion of mass of carbon and oxygen in carbon dioxide.
In CO\(_2\) , C : O = 12 : 32 or 3 : 8
In other words,
we can say that
12.00 g carbon reacts with oxygen = 32.00 g
3.00 g carbon will react with oxygen = \(\frac{32}{12}\) x 3 = 8g
Therefore, 3.00 g of carbon will always react with 8.00 g of oxygen to form CO\(_2\) (11g), even if large amount (50.00 g) of oxygen is present.
This answer will be governed by ‘the law of constant proportions’.
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