Indicate and explain the sign of ΔS_univ for each process. a. 2 H₂( g) + O₂( g) → 2 H₂O (l ) at 298 K.

Video transcript

Hello. Everyone in this video we're trying to find for the sign of our delta S. For the given reaction. So, from our starting material side we see that there's going to be three moles of gas reason being we have two moles of gas from our carbon monoxide and then we have Spread out that and then we have one mole of 02 gas here. So two plus one, that's going to be three moles of gas total on the starting material side. On a product side, we have two moles of carbon dioxide. Alright, whenever we have on the product side that there's less moles of gas than on this dark material. Said we have the sign of delta S being negative. So we have negative deltas. Alright, so we have a course a combustion reaction right over here. It's given to us. Let's go ahead and actually write that out. So, we have a combustion reaction which is actually also going to be a exo thermic reaction. And because of that, then our doctor H sign, it's going to be negative. So, we have our negative delta H and our negative delta us. And because we have both of these being negative and the reaction will only be spontaneous at low temperatures. And this is going to be my final answer for this problem. So, again, we have solved for our sign for delta S. And then this is going to be the rationale for this negative delta s. All right, Thank you all so much for watching