discover the typical enthalpy of development of ethylene, C2H4(g), given the following data: C2H4(g) + 3O2(g) --> 2CO2(g) + 2H2O(l) H°rxn = –1411 kJ provided that: H°f = –393.5 kJ/mol H°f = –285.8 kJ/mol

The traditional enthalpy of formation of ethylene, C2H4(g), given the over data, is H°f(C2H4(g) =52.4 kJ/mol.

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The warmth of reaction is the an outcome of the breaking of bonds within the reactant types and the reforming of bond to make the product species. The warm of formation (`Delta` H°f) is the power required to form a compound in kilojoules per mole that substance. Heats of formation can...


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The warmth of reaction is the result of the breaking of bonds within the reactant types and the reforming of bond to do the product species. The heat of formation (`Delta` H°f) is the energy required to type a compound in kilojoules every mole of substance. Heats of formation can be provided to calculation the heat of reaction (`Delta` H°rxn) by subtracting the heats of formation of the reactants from the heats of formation of the products:

Heat of reaction = Heats of formation of commodities - Heats of formation of reactants

Heats of development can be uncovered in tables such together the one discovered here. Aspects have a warm of development of zero (they are the structure blocks because that compounds). The heats that reaction room reported per mole of substance, so we"ll need to multiply the warm of development by the variety of moles of every substance in the reaction.

So, because that our reaction, C2H4(g) + 3O2(g) --> 2CO2(g) + 2H2O(l), us have:

H°rxn = 2 mol CO2(g) H°f(CO2(g)) + 2 mol H2O(g) H°f(H2O(g))

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Substituting the values for H°rxn and also H°f (remember H°f because that O2 is zero):

-1411 kJ = 2 mol (-393.5 kJ/mol) + 2 mol (-285.8 kJ/mol) -

Rearranging to fix for H°f(C2H4(g):

H°f(C2H4(g) = 2 mol (-393.5 kJ/mol) + 2 mol (-285.8 kJ/mol) + 1141 kJ

H°f(C2H4(g) =52.4 kJ/mol


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The warm of reaction of a specific chemical reaction deserve to be expressed as: