00:01
We're told that one of the following processes is spontaneous.
00:03
We have to indicate which one, either a, b or c, for a of h2o, changing state from liquid to gas at one atmospheric pressure.
00:20
So the reaction quotient is equal to the partial pressure of the h2o, which is equal to 1, delta g not for the reaction.
00:42
Is equal to the sum of delta g not for the products minus the sum delta g not for the reactants so we can look up these values here we have some of the sorry i'm going to squeeze in here n moles so one mole for the products negative 228 .6 kilojoules per mole minus one mole for the reactants, negative 237 .1 kilojoules per mole.
01:39
Delta g0 reaction works out to 8 .5 kilograms, or kilojoules, sorry.
01:47
And then we can calculate delta g0 is equal to delta g0 reaction plus rt lon q.
01:56
8 .5 kilojoules plus ideal gas constant.
02:01
8 .314 times 10 of the negative 3, kilojoules per mole kelvin, 2 .98 kelvin, lawn of 8 .5 kilojoules.
02:18
And this would give us 8 .5 kilojoules.
02:27
Or lawn, no, sorry, not lawn of 8 .5.
02:30
Their quotient here was long of 1.
02:39
So we get 8 .5 kilojoules.
02:42
Since delta g not is greater than zero, this is non -spontaneous.
02:51
So a is non -spontaneous.
02:56
So let's move on to b.
02:57
We have h2o liquid going to h2o gas, but this time i have 0 atmosphere.
03:12
The quotient is equal to the partial pressure of h2o, which is equal to 0 .1...