00:01
Problem 157 says to calculate the delta h for iodine chloride in its gaseous form at 25 degrees celsius.
00:10
The problem gives you the hint to use bond energies, which you can find in table 8 .5 in your textbook, and then additional properties in appendix 4.
00:22
So what we're trying to achieve here is the conversion of iodine in its gaseous form and chlorine in its gaseous form to icl.
00:51
Now if you start to think about the way this can be done mathematically, the first thing that probably comes to most, mind, as we've seen before in this chapter, is that iodine exists as molecular iodine, i2, and in a solid form.
01:14
So the first thing that we'll need to do then in order to get it to this gaseous form here is look at appendix 4 for the energy required for sublimation of solid iodine to gas.
01:37
Next, we'll have to take molecular iodine and molecular chlorine apart into single units of iodine and chlorine to put iodine chloride together.
01:55
So molecular iodine coming apart to two iodine atoms and the same thing for chlorine.
02:06
And of course, these, because they exist as diatomic molecules, breaking those apart, will require bond energies to go about solving this delta h mathematically.
02:43
So the bond energy we're looking for here is iodine bound to another iodine, here, a chlorine bound to another chlorine.
02:52
Finally, the last part of this is the two iodines in their gaseous form coming together with two chlorines to form these two iodine chlorides.
03:14
And again, we're looking at a bond energy, specifically the bond energy for iodine chloride...
