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?
1 mole of C = 12 g
1 mole of O2 = 32 g
C + O2 → CO2
12 g + 32 g → 44 g
4 4 4
[3g + 8g - 11g] → constant
8 g of O2 will be consumed from 50g of O2 and 42 g of O2 will be unreactive. It shows that 12 g of carbon burns in 32 g oxygеn from 44 g of CO2 bесоuse 3 g of carbon reacts with 8 g of oxygen to form 11 g of CO2. The same is given to us. Consequently 11.0 g of CO2 will be formed when 3.0 g of carbon is burnt in 50 g of oxygen consuming 8 g of O2, leaving behind 42 g of O2. The answer governs the Law of constant Proportion.
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