Assume that 3.33 x 106 kJ are needed to heat a swimming pool. If this energy is derived from the combustion of methane (CH4) at standard conditions (25 oC and 1 atm) what volume in liters of methane must be burned?
The heat of combustion of methane is 889.967 kJ/mol. The density of methane is 0.0680 kg/m3
thank you!
2007-02-01 09:23:23 · 3 answers · asked by Jessica R 1 in Science & Mathematics ➔ Chemistry
Insufficient information. What is the volume of the pool? To and from what temperature is it heated?
2007-02-01 09:35:29 · answer #1 · answered by gebobs 6 · 0⤊ 0⤋
3.33E6 kJ/889.967 kJ/mol = 3742 mol CH4
3742 mol * 16.05 gCH4/mol / 1000 g/kg = 60.05 kg CH4
60.05 kg / 0.0680 kg/m3 * 1000 dm3/m3 = 8.83 x 10^5 dm3 (L)
2007-02-01 17:42:43 · answer #2 · answered by smalltownwhiteboy 2 · 0⤊ 0⤋
880402.76
2007-02-01 17:47:05 · answer #3 · answered by suzzie 1 · 0⤊ 0⤋