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Problem: Use the bond dissociation energies Table 7.1 to calculate an approximate ΔH o (in kilojoules) for the reaction of ethylene with hydrogen to yield ethane.H2C=CH2(g)+H2(g) → CH3CH3(g)

🤓 Based on our data, we think this question is relevant for Professor Raghavachari & Jarrold's class at IU.

FREE Expert Solution

We're asked to calculate an approximate ΔHo (in kilojoules) for the reaction of ethylene with hydrogen to yield ethane:


H2C=CH2(g) + H2(g) → CH3CH3(g)


Recall that we can solve for the ΔH°rxn using bond energies, using the equation:


H°rxn=Hbond,reactants-Hbond,products


To do that, we need to do these steps:


Step 1: Draw the Lewis structure of each compound and determine the type of bonds present 

Step 2: Solve for ΔH°rxn using the given bond energies


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Problem Details

Use the bond dissociation energies Table 7.1 to calculate an approximate ΔH o (in kilojoules) for the reaction of ethylene with hydrogen to yield ethane.

H2C=CH2(g)+H2(g) → CH3CH3(g)

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 Raghavachari & Jarrold's class at IU.