To calculate the enthalpy of the reaction, we need to use the standard enthalpies of formation given in the table.
Reactants:
2C (s, graphite) = 2(0 kJ/mol) = 0 kJ/mol
H2 (g) = 0 kJ/mol
Products:
C2H2 (g) = 226.73 kJ/mol
ΔH rxn = ΣΔHf(products) - ΣΔHf(reactants)
ΔH rxn = 226.73 kJ/mol - (0 kJ/mol + 0 kJ/mol)
ΔH rxn = 226.73 kJ/mol
Therefore, the enthalpy of the reaction is 226.73 kJ.
Consider the reaction.
2 upper C (s, graphite) plus upper H subscript 2 right arrow upper C subscript 2 upper H subscript 2 (g).
Standard Enthalpies of Formation
Substance
DHf (kJ/mol)
C2 H2 (g)
226.73
CaCO3 (s)
–1206.92
CaO (s)
–635.09
CO (g)
–110.525
CO2 (g)
–393.509
H 2 O (I)
–285.8
H 2 O (g)
–241.818
C (s), diamond
1.895
C (s), graphite
0.0
Based on the equation and the information in the table, what is the enthalpy of the reaction?
Use Delta H r x n equals the sum of delta H f of all the products minus the sum of delta H f of all the reactants..
–453.46 kJ
–226.73 kJ
226.73 kJ
453.46 kJ
1 answer
1 answer