A certain compound was found to have a molar mass of 72.106 g. A 1.825 g sample of this compound was burned in pure oxygen gas. The measured amount of CO2 produced was 4.455 g, while that of H2O was 1.824 g. No other products were produced in the reaction.
How many moles of hydrogen were in the original sample that underwent combustion ?
2007-04-02 09:11:16 · 2 answers · asked by ashleyjohn18 1 in Science & Mathematics ➔ Chemistry
To get the moles of hydrogen, take the mass of water that was formed, and convert that to moles of water. Since there are 2 moles of H in each mole of water, multiply the moles of water formed by 2 to get the moles of hydrogen. That value should be the moles of hydrogen in your original sample, since the only place hydrogen could have come from was the original compound.
2007-04-02 09:17:16 · answer #1 · answered by hcbiochem 7 · 0⤊ 0⤋
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2016-05-16 09:15:37 · answer #2 · answered by Anonymous · 0⤊ 0⤋