Consider the following reaction: 2CH3OH(g)→2CH4(g)+O2(g)ΔH=+252.8kJ 1) Calculate the amount of heat transfer?
Consider the following reaction:
2CH3OH(g)→2CH4(g)+O2(g)ΔH=+252.8kJ
1) Calculate the amount of heat transferred when 29.0
g of CH3OH(g) is decomposed by this reaction at constant pressure.
2.)For a given sample of
CH3OH, the enthalpy change during the reaction is 82.6kJ . How many grams of methane gas are produced?
3.)How many kilojoules of heat are released when 38.1
g of CH4(g) reacts completely with O2(g) to form CH3OH(g) at constant pressure?
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Verified answer
2CH3OH(g) → 2CH4(g) + O2(g) ΔH = +252.8kJ
OR CH3OH(g) → CH4(g) + 1/2O2(g) ΔH = +126.4kJ
1 mol 1 mol 1/2 mol
1) 29.0 g of CH3OH = 29.0/32 = 0.906 mol of CH3OH
So the heat transfer = 0.906 x 126.4 = 114.52 kJ
2) As when +126.4 kJ enthalpy change takes place 1 mol of CH4 is produced.
So 82.6 kJ enthalpy change will produce 82.6/126.4 = 0.65 mol of CH4 = 0.65 x 16 = 10.4 g of CH4
3) 38.1 g of CH4 = 38.1/16 = 2.38 mol of CH4
Heat released = 2.38 x 126.4 = 300.83 kJ