CH4g + O2g ---- CO2g + H20g
How mwany grams of water formed during the combustion of 0.264 moles CH4?
2006-11-29 12:35:43 · 6 answers · asked by freemanjr2 1 in Science & Mathematics ➔ Chemistry
Since it takes 1 mole of O2 to react with H4 and get H2O + H2O. I would have to say that .264 moles of H2O were created. water is 18gper mole so .264*18g=4.752g of water.
2006-11-29 12:41:20 · answer #1 · answered by hockey 2 · 0⤊ 0⤋
The chemical reaction is actually CH4 + 2O2 ===> CO2 + 2H2O. Begin with 0.264mol CH4. Multiply by 2molH2O/1molCH4. That comes from the balanced equation. The molCH4 cancel, leaving molH2O. Multiply by 18gH2O/1molH2O. That comes from the molecular weight of water, 1 + 1 + 16 = 18. The molH2O cancel, leaving gH2O, which is the answer.
2006-11-29 12:44:10 · answer #2 · answered by steve_geo1 7 · 0⤊ 0⤋
mixture and addition are the two names used to describe this reaction. Synthesis has been used, besides the undeniable fact that it oftentimes refers to a reaction this is used to make a definite product (and there could be greater effective than one product).
2016-12-10 18:46:08 · answer #3 · answered by ? 4 · 0⤊ 0⤋
(0.246 moles CH4)(1mole/16 g)= .0153 moles CH4( 2mole H2o/1mole CH4) = .0306molesH2O x 18 g/mole = .551 grams
2006-11-29 12:48:03 · answer #4 · answered by Robert O 2 · 0⤊ 0⤋
4.752
just multiply .264 by the molar mass of water which is 18g
2006-11-29 12:39:29 · answer #5 · answered by Alex P 2 · 0⤊ 0⤋
idunno
2006-11-29 12:37:42 · answer #6 · answered by Anonymous · 0⤊ 1⤋