Home / Questions / The methane molecule, CH4, has the geometry shown in Figure 2.17. Imagine a hypothetical p...
The methane molecule, CH_{4}, has the geometry shown in Figure 2.17. Imagine a hypothetical process in which the methane molecule is “expanded,” by simultaneously extending all four C—H bonds to infinity. We then have the process
CH_{4}(g) C(g) + 4 H(g)
(a) Compare this process with the reverse of the reaction that represents the standard enthalpy of formation of CH_{4}(g). (b) Calculate the enthalpy change in each case. Which is the more endothermic process? What accounts for the difference in ∆H° values? (c) Suppose that 3.45 g CH_{4}(g) reacts with 1.22 g F_{2}(g), forming CH_{4}(g) and HF(g) as sole products. What is the limiting reagent in this reaction? If the reaction occurs at constant pressure, what amount of heat is evolved?
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