Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: aaronstonedd on April 19, 2013, 12:32:50 PM
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The numerical in it's full glory:
10 mL (sic) of hydrogen combine (sic) with 5 mL (sic) of oxygen to yield water. When 200 mL (sic) of hydrogen at NTP are (sic) passed over heated CuO, the latter loses 0.144 g of its mass. Do these results agree with the law of constant composition?
- Do hydrogen and oxygen refer to
(i) "H" and "O", or
(ii) "H2 and O2, or
(iii) "H2 and O? - What results are we supposed to expect, that can clarify whether "these results" agree with the law of constant proportions?
What is the step-by-step procedure we have to follow to get "the results ... we are supposed to expect"?
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H2 (sic) and O2 (sic).
Apparently you should check if the oxygen/hydrogen proportion is identical in each case (sic).
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Dear OP, I think you have fallen afoul of Muphry's Law in your use of "it's" and your many, many uses of "sic".
It isn't correct to ask the internet for a step by step procedure to figure out your results; part of the question is whether you can figure that out, I think.
So, let me ask you this in turn; what chemical reaction is going on here? Write its balanced equation.
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I think you can assume that H2 and O2 are being used. These gasses are diatomic, we can't "pass over" or "combine" H and O. Those may be used to visualize reactions, but they're not things we can measure. A tank full of hydrogen or oxygen, we can measure those as full or empty, and they'll contain diatomic gasses.