Combustion analysis of 1.00g of testosterone yields 2.90g of CO2 and .875g H2O. What are the mass percents of carbon, hydrogen, and oxygen in testosterone?
If 7.35g of chromium reacts directly with oxygen to form 10.74g of a metal oxide, what is the simplest formula of the metal oxide? name the oxide.
If 7.35g of chromium reacts directly with oxygen to form 10.74g of a metal oxide, what is the simplest formula of the metal oxide? name the oxide.
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The second is easy. The first, I'm still working on.
7.35g of Cr means we have ~0.14mol of Chromium present. 3.39g of oxygen means we have ~0.21mol present.
There is ~1.5 times as much oxygen as Chromium meaning the simplest stoichiometric ratio is 2(Cr):3(O) and the formula is therefore Cr2O3 with the name Chromium (III) Oxide.
I have no easy solution to the first problem without first knowing the relative formula mass of testosterone. Or if that's not possible, the number of moles of oxygen used in the combustion.
7.35g of Cr means we have ~0.14mol of Chromium present. 3.39g of oxygen means we have ~0.21mol present.
There is ~1.5 times as much oxygen as Chromium meaning the simplest stoichiometric ratio is 2(Cr):3(O) and the formula is therefore Cr2O3 with the name Chromium (III) Oxide.
I have no easy solution to the first problem without first knowing the relative formula mass of testosterone. Or if that's not possible, the number of moles of oxygen used in the combustion.
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I figured out the first problem. It should be 89% Carbon, 9.7% Hydrogen and 1.3% Oxygen.
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The answer lies by knowing that chromium times oxygen form then divid e by CO2
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the.......****?