A swimming pool, 10.0 m by 4.0 m, is filled with water to a depth of 3.0 m at a temperature of 20.2°c. if the energy needed to raise the temperature of the water to 29.7°c is obtained from the combustion of methane (ch4), what volume of methane, measured at stp, must be burned? ∆hcombustion for ch4 = - 891 kj/mol

Question

Physics

Malachi Shepherd

1 May, 02:06

A swimming pool, 10.0 m by 4.0 m, is filled with water to a depth of 3.0 m at a temperature of 20.2°c. if the energy needed to raise the temperature of the water to 29.7°c is obtained from the combustion of methane (ch4), what volume of methane, measured at stp, must be burned? ∆hcombustion for ch4 = - 891 kj/mol

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Reese May · Answer 1

You need to find the mass of water in the pool.

Find the volume (10 x 4 x 3) = 120 m3

Water has a density of 1000g/m3, so 120 m3 = 120 x 1000 = 120 000 kg

[delta]H = 4.187 x 120 000 x 3.4 (and the units will be kJ)

You then use the heat of combustion knowing that each mole of methane releases 891 kJ of heat so if you divide 891 into the previous answer, you will get the number of moles of CH4