00:01
In this problem, we want to explain how the relative amounts of each one of the reactants, given reactions compare as a result of increasing the volume in which these reactions occur.
00:14
We know that when we increase the volume, that means that we are decreasing the pressure.
00:19
And we also know that lechatlier's principle will respond to that disturbance of a decrease in pressure by increasing the pressure in order to reestablish equilibrium.
00:28
We also know that higher pressures are a result of a greater amount of gaseous species because we add all of the partial pressures of each one of those gases together to get the total pressure.
00:46
So that means that when we increase the volume, which results in a decrease in pressure, we need to increase the pressure by forming more moles of gas.
00:56
So whichever side of the reaction has more moles of gas, that's the side which will be favored in each one of these reactions.
01:06
So in part a, we just have methanol as a liquid, and so there are no gaseous molecules on that side, and we are forming one mole of gaseous methanol...