Question 16.3: CALCULATING THE STANDARD ENTROPY OF REACTION Calculate the s...
CALCULATING THE STANDARD ENTROPY OF REACTION
Calculate the standard entropy of reaction at 25 °C for the Haber synthesis of ammonia:
N2(g) + 3 H2(g) → 2 NH3(g)STRATEGY
To calculate ΔS° for the reaction, subtract the standard molar entropies of all the reactants from the standard molar entropies of all the products. Look up the S° values in Table 16.1 or Appendix B, and remember to multiply the value for each substance by its coefficient in the balanced chemical equation.
TABLE 16.1 Standard Molar Entropies for Some Common Substances at 25 °C
Substance Formula S°[J/K · mol)] | Substance Formula S°[J/K · mol)] |
Gases
Acetylene C2H2 200.8 Ammonia NH3 192.3 Carbon dioxide CO2 213.6 Carbon monoxide CO 197.6 Ethylene C2H4 219.5 Hydrogen H2 130.6 Methane CH4 186.2 Nitrogen N2 191.5 Nitrogen dioxide NO2 240.0 Dinitrogen tetroxide N2O4 304.3 Oxygen O2 205.0 |
Liquids
Acetic acid CH3CO2H 160 Ethanol CH3CH2OH 161 Methanol CH3OH 127 Water H2O 69.9 Solids Calcium carbonate CaCO3 91.7 Calcium oxide CaO 38.1 Diamond C 2.4 Graphite C 5.7 Iron Fe 27.3 Iron(III) oxide Fe2O3 87.4 |
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ΔS° = 2 S°(NH3) – [S°(N2) + 3 S°(H2)]
= (2 mol)(192.3 K ⋅ molJ) – [(1 mol)(191.5K ⋅ molJ)+ (3 mol)(130.6K ⋅ molJ)]
= -198.7 J/K
BALLPARK CHECK
As predicted in Worked Example 16.1c, ΔS° should be negative because the reaction decreases the number of gaseous molecules from 4 mol to 2 mol.