00:01
So in this question, we are asked to determine whether or not the vaporization of methanol is spontaneous at 80 degrees celsius in one atmosphere.
00:14
So what we're going to do is we will find the enthalpy of the reaction using this formula.
00:22
So we're going to add the enthalpy of formation under the standard states of the products.
00:28
And then we'll subtract the enthalpy of formation in the standard state of the react.
00:34
So our product is going to be methanol in the vapor phase and the reactant of methanol in the liquid phase.
00:45
So then we're going to get the enthalpyofor formation values for these two and plug it into this formula.
00:52
Then we end up getting the enthalpy of reaction in kilojoules, and we need to convert that to joules so multiply by a thousand.
01:01
Then we're going to find the change in entropy under standard states.
01:07
So we're going to use a similar format except now we're looking at the entropy under standard states of products and reactants.
01:17
So we are going to look that up in the appendix.
01:21
And again, the product is going to be the methanol in the gaseous state and the reactant will be methanol in the liquid state...