The conversion of natural gas, which is mostly methane, into products that contain two or more carbon atoms, such as ethane (C2H6), is a very important industrial chemical process. In principle, methane can be converted into ethane and hydrogen:
2 CH4(g)→C2H6(g) + H2(g)
In practice, this reaction is carried out in the presence of oxygen:
2 CH4(g) + ½O2(g)→C2H6(g) + H2O(g)
(a) Using the data in Appendix C, calculate K for these reactionsat 25 °C and 500 °C. (b) Is the difference in ΔG° for thetwo reactions due primarily to the enthalpy term (ΔH) or theentropy term (-TΔS)? (c) Explain how the preceding reactionsare an example of driving a nonspontaneous reaction, asdiscussed in the “Chemistry and Life” box in Section. (d)The reaction of CH4 and O2 to form C2H6 and H2O must becarried out carefully to avoid a competing reaction. What isthe most likely competing reaction?
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