Problem: The methane molecule, CH4, has the geometry shown in following figure. 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 CH4(g) → C(g) + 4 H(g).Compare this process with the reverse of the reaction that represents the standard enthalpy of formation of CH4(g). Which is the more endothermic process?

FREE Expert Solution

CH4(g) → C(g) + 4 H(g).

• involves one compound forming two species→ bond breaking
 endothermic


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Problem Details
The methane molecule, CH4, has the geometry shown in following figure. 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 CH4(g) → C(g) + 4 H(g).

The figure shows a ball-and-stick model and a perspective drawing of CH4.

Compare this process with the reverse of the reaction that represents the standard enthalpy of formation of CH4(g). Which is the more endothermic process?

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