00:02
So nitricin dioxide is one of the pollutants in the atmosphere.
00:08
I work too, that i react with one which is called nitricarsive.
00:11
So this would be 3 -102 gas plus h2 or liquid gas, liquid, going to hno3, occurs, plus anode gas.
00:33
So we are told that the, we are turned to do what? to calculate the delta g and the kp, which is the equilibrium constant at 25 degrees celsius, and we should comment on the spontaneity of the reaction.
00:51
So we can calculate the delta g for the reaction by saying the delta g of the formation of the products minus the delta g of formation of each of the reactant.
01:02
So we have two moles of hnl3, multiplied by the dltdltg, g of formation of h &l3, which is minus 110 .9 kilojoules per mole, plus one mole of n whole, one of n hold, multiplied by the dlta g of formation of n hole, which is, you have to check that up on the table, which is 87 .6, 87 .6 kilojouge per mole.
02:12
Minus we have three moles of no2 three mole times the dltg of formation of no2 is 51 .3 51 .3 kg a mole plus one more of water multiplied by the dltg of water and that is that's minus to 1030 that's minus 2 .37, minus 2 .37, 2 .37.
03:20
2 .37 .2 .37.
03:26
1 .2.
03:27
Then we can go ahead and evaluate that.
03:36
Okay...