Here it says determine the change in the entry of the universe for the following reaction at 32°C. So here they're giving us this chemical reaction and we're going to say that our enthalpy of the reaction change in enthalpy of our reaction is -140 kilojoules and the entropy of our reaction is 3.6 joules per Kelvin.
So remember here that our total change in entropy, which is the same thing as the entropy of our universe, equals the change in the entropy of our surroundings plus the change in the entropy of our reaction. Here we already know that changing entropy of our reaction. That's 3.6 Joules per Kelvin. What we need to do is determine the change in the entropy of our surroundings, which remember is equal to negative delta H of R reaction divided by temperature in Kelvin.
So we're going to take that number and plug it in and we're going to say here, since entropy change of our reaction is in joules, I'm going to convert these kilojoules into joules by multiplying them by 1000 temperature. We add 273.15 to this 32°C and that gives me 305.15 Kelvin. So we have a negative of a negative. Remember the negative was already there, and then we have an additional negative.
Here the change in the entropy of my surroundings will be a positive value. It comes out to be +458.79 Joules per Kelvin. We take that and we plug it here into our formula and now we're going to have the change in the entropy of our universe, or total. That comes out to a +462.39 Joules per Kelvin. So this would be our final answer.
Δ S = Δ S + Δ S Δ S = - Δ H T