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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:

H°rxn=Hbond reactants-Hbond products


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.

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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

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Bond Energy concept. If you need more Bond Energy practice, you can also practice Bond Energy practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Greenberger's class at PSU.