Asked by Luke
For the reaction:
CH4(g) + 2O2(g)-->CO2(g)+2H2O (l)
ÄH = -50.38 kJ/mol,
How many moles of methane (CH4) must be burned to produce 137 kJ of heat?
CH4(g) + 2O2(g)-->CO2(g)+2H2O (l)
ÄH = -50.38 kJ/mol,
How many moles of methane (CH4) must be burned to produce 137 kJ of heat?
Answers
Answered by
kyle
For each mole of CH4 reacted there is 50.38 kj released.
137 kj * (1 mol/50.38 kj) = 2.719 moles of CH4. 4 sig figs
additional info: 50.38 is positive because it's asking how much heat is produced (released) and if you say -50.38 kj is released it's like a double negative.
137 kj * (1 mol/50.38 kj) = 2.719 moles of CH4. 4 sig figs
additional info: 50.38 is positive because it's asking how much heat is produced (released) and if you say -50.38 kj is released it's like a double negative.
Answered by
jojo
i need help
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