what is the mass in kg of CO2 formed by combusting enough fuel to release 1.0 kJ of energy for this equation?
CH4 + 2O2 -> CO2 + 2H2O
CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)
Hrxn = H0f products - H0f reactants
= 2*-285.83-393.5 -(-74.81+2*)
= -890.35KJ/mole
CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) Hrxn = -890.35KJ/mole
1 mole of CO2 produce to released -890.35KJ
-890.35 Kj energy is released from 1 mole of CO2
-890.35 Kj energy is released from 44g of CO2
1KJ energy is released from = 44*1/890.35 = 0.05g of CO2
0.05g of CO2= 5*10^-2 g of CO2
= 5*10^-5Kg of CO2>>>>>answer
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