Final answer:
Using the balanced equation for the combustion of ethane, 600 cc of ethane requires 2100 cc of oxygen. With 2500 cc of oxygen available, the unused volume of oxygen is 2500 cc - 2100 cc = 400 cc. The volume of carbon dioxide formed is 2 x 600 cc = 1200 cc, so none of the provided options is correct.
Step-by-step explanation:
To determine the volumes of unused oxygen and carbon dioxide formed when 600 cc of ethane is burnt with 2500 cc of oxygen, we need to consider the balanced chemical equation for the combustion of ethane (C2H6):
C2H6 + 3.5 O2 → 2 CO2 + 3 H2O
This equation indicates that 1 volume of ethane reacts with 3.5 volumes of oxygen to produce 2 volumes of carbon dioxide and 3 volumes of water as in the water vapor form. Using Avogadro's law, which states equal volumes of gases at the same temperature and pressure contain the same number of molecules, we can infer the reaction ratios:
For 600 cc of ethane, the oxygen required for complete combustion would be 600 cc x 3.5 = 2100 cc.
Since 2500 cc of oxygen is provided and only 2100 cc is required, the unused volume of oxygen would be 2500 cc - 2100 cc = 400 cc.
The volume of carbon dioxide formed is twice the volume of ethane burnt, so it would be 2 x 600 cc = 1200 cc.
Therefore, none of the given options is correct.