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