Concept explainers
Acetylene (C2H2) and nitrogen (N2) both contain a triple bond, but they differ greatly in their chemical properties.
a. Write the Lewis structures for the two substances.
b. By referring to Appendix C, look up the enthalpies of formation of acetylene and nitrogen. Which compound is more stable?
c. Write balanced chemical equations for the complete oxidation ofN2 to form N205(g) and of acetylene to form C02(g) and H20(g).
d. Calculate the enthalpy of oxidation per mole for N2 and for C2H2 (the enthalpy of formation of N205(g) is 11.30k.J/m01).
e. Both N2and C2H2 possess triple bonds with quite high bond enthalpies
(Table 8.3 C).
Calculate the enthalpy of hydrogenation per mole for both compounds:acetylene plus 1-12 to make methane, CH4; nitrogen plus H2 to make ammonia, NH3.
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CHEMISTRY THE CENTRAL SCIENCE 14TH EDI
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