document.write( "Question 826356: How many liters of water vapor can be produced if 8.9 liters of methane gas (CH4) are combusted, if all measurements are taken at the same temperature and pressure? Show all of the work used to solve this problem.
\n" ); document.write( "CH4 (g) + 2 O2 (g)yields CO2 (g) + 2 H2O (g \n" ); document.write( "

Algebra.Com's Answer #498056 by KMST(5328) $\"\"$ $\"About$

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As 1 mole of methane reacts, 2 moles of water are produced.
\n" ); document.write( "That's what the balanced equation for that reaction tells you,
\n" ); document.write( "because there is an implied 1 in front of $\"CH%5B4%5D\"$ (methane),
\n" ); document.write( "and a 2 in front of $\"H%5B2%5D\"$ $\"O\"$ (water).
\n" ); document.write( "If all the reactants and products are gases,
\n" ); document.write( "at the same temperature and pressure,
\n" ); document.write( "and those conditions are such that all the reactants and products behave as ideal gases,
\n" ); document.write( "one mole of each occupies the same volume.
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\n" ); document.write( "As the number of moles of water produced is double the number of moles of methane reacting,
\n" ); document.write( "the volume of water produced will be twice the volume of methane reacting.
\n" ); document.write( "So $\"2%2A8.9L=highlight%2817.8L%29\"$ of water vapor will be produced.
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\n" ); document.write( "NOTES:
\n" ); document.write( "1) We could calculate how many moles of methane are in 8.9L of methane if we knew the temperature and pressure, but that is not needed (or possible) for this problem.
\n" ); document.write( "2) For chemistry questions, try the mychemistrytutor website. It used to provide very fast and correct answers when I used to answer questions there. \n" ); document.write( "

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