PDF chapter test TRY NOW
Answer the following 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 combination will govern your answer?
\(C\) + \(O_2\) → \(CO_2\)
Carbon 1 mole 12 g + Oxygen 1 mole 32 g →
It shows that 12 g of carbon burns in 32 g of oxygen form 44 g of carbon dioxide. Hence, of carbon reacts with 8 g of oxygen to form 11 g of carbon dioxide. It is given that 3.0 g of carbon is burnt with 8 g of oxygen to produce 11.0 g of \(CO_2\).
Therefore, 11.0 g of carbon dioxide will be formed when 3.0 g of \(C\) is burnt in 50 g of oxygen, consuming 8 g of oxygen, leaving behind 50 - 8 = of \(O_2\). The answer governs the .
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