(b) Based on average bond enthalpies, would you expect a photon capable of dissociating a C-Cl bond to have sufficient energy to dissociate a C-Br bond?

Video transcript

Hi everyone for this problem, we're told to consider a photon with enough energy to break a nitrogen nitrogen bond. Will the same photon be able to break a nitrogen hydrogen bond based on average bond and throw peas? Okay, so we're going to need to know what the bond entropy is for our nitrogen nitrogen bond and our nitrogen hydrogen bond in order to solve this problem. So we can go ahead and look up those values. And for our nitrogen nitrogen bond, The average bond antelope is for our nitrogen hydrogen bond, The average bond entropy is and both of these are in kila jewels per mole. Okay, so as we can see the nitrogen hydrogen bond has a higher bond entropy, which means it's going to need more energy than the nitrogen nitrogen needs to break. So the answer to this question is going to be no. Okay, this photon will not have enough energy to break the nitrogen hydrogen bond. Okay, so that's the end of this problem. I hope this was helpful.