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Unformatted text preview: 2 O would be produced from 1.57 moles of O 2 (assuming the hydrogen gas is not a limiting reactant)? The ratio is the stoichiometric relationship between H 2 O and O 2 from the balanced equation for this reaction. For the combustion of butane (C 4 H 10 ) the balanced equation is: Calculate the mass of CO 2 that is produced in burning 1.00 gram of C 4 H 10 . First of all we need to calculate how many moles of butane we have in a 100 gram sample: now, the stoichiometric relationship between C 4 H 10 and CO 2 is: , therefore: The question called for the determination of the mass of CO 2 produced, thus we have to convert moles of CO 2 into grams (by using the molecular weight of CO 2 ): Thus, the overall sequence of steps to solve this problem were: In a similar way we could determine the mass of water produced, or oxygen consumed, etc. 1996 Michael Blaber...
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 Spring '10
 puteri
 Mole, Stoichiometry, Chemical reaction, Moles, balanced equations

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