Question

When 6.0 g of carbon is burnt in 16.00 g oxygen, 22.00 g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 6.00 g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combination will govern your answer? Name and define the law.(2 marks)​
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Answer 1

Answer:

22 g of CO2 will be formed when 6 g of carbon is burnt in 32 g of oxygen. The atomic mass of C is 12 g/mol. The molecular masses of O2 and CO2 are 32 g/mol and 44 g/mol respectively. 12 g C will combine with 32 g O2 to form 44 g CO2.

Answer 2

Given:

6 g of Carbon reacts with 16g of oxygen to form 22 gm of CO2.

For second case,

6 g of carbon is burned with 50 g of oxygen.

To find:

How much CO2 is evolved in second case.

Law of chemical combination that governs this question.

Solution:

The law of combination which governs this question is LAW OF DEFINITE PROPORTIONS.

It states that," every chemical compound contains fixed and constant proportions (by mass) of its constituent elements."

• Explanation with respect to the above question,

for the formation of CO2 molecule.

• 1 carbon mole combines with 1 dioxygen mole to for 1 mole of CO2.
• C + 02 ----> CO2
• In first case, 6 g of carbon( that is half mole of carbon) reacts with 16 g of oxygen (that is half mole of dioxygen) forms 22 g( that is half mole of CO2)
• ½C + ½O2 -----> ½CO2
• Here, the proportion remains constant even if the quantity remains same.
• For the second case, we have 6g of carbon (½ mole) and 50g of dioxygen which is 1.5625 moles.
• Since we require only half mole of dioxygen for half mole of carbon (limiting reactant) only half mole of dioxygen will be used and remaining mole will remain excess.
• So, half mole of carbon will be burnt with half mole of dioxygen to form half mole that is 22g of carbon dioxide.

Hence,the carbon dioxide produced is 22g