Trenda M.

asked • 11/21/14

Thermochemistry: Heating water with Methane

I'm stuck on this one
How many grams of methane must be combusted to heat 1.00 kg of water from 25.0 °C to 90 °C, assuming H2O(l) is the product of the reaction and no heat is lost to the surroundings?
So far I have 
1000 g H2O
ΔT = 65.0 °C
q = 0
CH(g) + 2O2 (g) → 2H2O (l) + CO2
heat evolved = 4.1798 J g-1 °C-1 (1000g)(65.0°C)(1kJ/1000J) = 271.6 kJ

1 Expert Answer


Yohan C. answered • 11/22/14

4 (1)

Math Tutor (up to Calculus) (not Statistics and Finite)

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