Question

Use the given average bond dissociation energies to estimate ΔE (kJ) for the reaction of methane, CH4(g), with fluorine according to the equation below. Enter your answer as the nearest whole number without units. CH₄(g) + 2 F₂(g) → CF₄(g) + 2 H₂(g)

Answer 1

To estimate ΔE for the reaction of methane with fluorine, we need to consider the average C-H bond energy. Using the given information, we can calculate the total energy required to break the four C-H bonds in methane.

Step-by-step explanation:

To estimate ΔE for the reaction of methane with fluorine, we need to consider the bond energies involved. From the given information, the average C-H bond energy is 415 kJ/mol. We can use this value to calculate the energy required to break the four C-H bonds in methane. The reaction equation shows that two moles of F2 molecules are required to react with one mole of methane. Since there are four C-H bonds in methane, we multiply the average bond energy by four to get the total energy required to break the C-H bonds. So ΔE = 4 * 415 kJ/mol = 1660 kJ/mol.