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A certain compound contains only C, H, and N. Combustion of 0.125 g of this compound...
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The compound contains only carbon C, hydrogen H and nitrogen N. When 0.125 g of the compound undergoes combustion 0.172 g of H2O and 0.279 g of CO2 are produced.
The atomic mass of hydrogen is 1 and that of oxygen is 16. H2O has a molecular mass of 2 + 16 = 18 g/ mole. 0.172 g of water (H2O) is equivalent to 0.172/18 = 9.55*10^-3 moles of H2O
The molecular mass of carbon is 12 and that of oxygen is 16. The molecular mass of CO2 is 12 + 16*2 = 44 g/mole. 0.279 g of CO2 is equivalent to 6.34*10^-3 moles of CO2.
Posted by justaguide on June 28, 2013 at 5:43 PM (Answer #1)
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Number of moles = given mass / molecular mass
No. of moles of H2O= .172 / 18 = .0095556 moles
No. of moles of CO2 = .279 / 44 = .0063409 moles
Posted by smart-kavya on July 1, 2013 at 10:04 AM (Answer #2)
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