What is the change in heat (in kJ) when 4.50 g of methane gas is burned...
What is the change in heat (in kJ) when 4.50 g of methane gas is burned in a constant-pressure system? The enthalpy of the given reaction is ΔH = -890 kJ. CH4(g) + 2 O2(g) --> CO2(g) + 2 H2O(l)
Homework Answers
Since this is exothermic reaction the heat liberated when 1 mol (16.04 g) of methane burnt is given 890 kJ
Therefore amount of heat liberated on combustion of 4.5 g of methane is
= (890 kJ x 4.5) / 16.04 = 249.69 kJ
Therefore the change in heat when 4.5 g of methane gas burner under constant pressure system is 249.69 kJ
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What is the change in heat (in kJ) when 4.50 g of methane gas is
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