# Problem: Use the given bond enthalpies to estimate ∆H for the following reaction:CH4(g) + 2 F2(g) → CF4(g) + 2 H2(g)Bond enthalpies:C−F 450. kJ mol−1    C−H 410. kJ mol−1     F−F 158 kJ mol−1     H−H 436 kJ mol−1(A) 318 kJ (B) 716 kJ (C) -358 kJ (D) -716 kJ (E) -318 kJ

###### FREE Expert Solution

We’re being asked to calculate the enthalpy (ΔH) of reaction (in kJ) for the given reaction using the given bond enthalpies.

CH4(g) + 2 F2(g) → CF4(g) + 2 H2(g)

To calculate the ΔH°rxn using bond energies, we’re going to use the following equation:

Let’s first figure out what kind of bonds and how many moles are present in each reactants and products because the given bond energies are per mole.

Draw the structure of each compound.

82% (86 ratings) ###### Problem Details

Use the given bond enthalpies to estimate ∆H for the following reaction:

CH4(g) + 2 F2(g) → CF4(g) + 2 H2(g)

Bond enthalpies:

C−F 450. kJ mol−1    C−H 410. kJ mol−1     F−F 158 kJ mol−1     H−H 436 kJ mol−1

(A) 318 kJ

(B) 716 kJ

(C) -358 kJ

(D) -716 kJ

(E) -318 kJ