“…Methane, the simplest hydrocarbon, has emerged as an attractive source of both carbon and energy because its annual production has continued to grow since the shale gas revolution that commenced in the United States in 2006. − This gaseous hydrocarbon has been consumed directly as fuel, but another important approach is to transform it into a variety of platform chemicals widely employed in the chemical industry. Methane reactions include steam/dry reforming to produce a synthesis gas (i.e., a mixture of CO and H 2 ); partial oxidation to obtain CO, methanol, and formaldehyde; halogenation to provide methyl halides; and dehydroaromatization to synthesize benzene. − ,,, Other examples are coupling reactions under oxidative/nonoxidative conditions to synthesize light paraffins and olefins directly from methane, where both reactions proceed exothermically and thus favor low reaction temperatures. − ,− ,− Under oxidative conditions, such mild reaction conditions are also beneficial for the suppression of undesired side reactions involving the complete oxidation of methane and desired hydrocarbon products to CO 2 as well as coke formation. However, the extremely high dissociation energy of the C–H bonds of methane (ca.…”