Please let me know if you need any clarification. I'm always happy to answer your questions.

Q=T(delta s)

heat of vaporization for 1 mol=230kj

so heat of vaporization for 1 mol=230*2=460KJ

460*10^3 J=(2270+273)delta S

delta S=460*10^3/(2270+273)

delta S=180.89 J/K

so entropy change 180.89 J/K

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Please let me know if you need any clarification. I'm always happy to answer your questions.

Using standard thermodynamic data at 298K, calculate the entropy change for thesurroundings when 1.89 moles of Fe_{3}O_{4}(s) react at standard conditions. S°_{surroundings} = J/K

2SO_{2}(g) + O_{2}(g)2SO_{3}(g)

Using standard thermodynamic data at 298K, calculate the entropy change for thesurroundings when 2.15 moles of SO_{2}(g) react at standard conditions. S°_{surroundings} = J/K

to find delta H you have to find the enthalpy change of the reaction.to do that you have to use standard thermodynamic data from book.at this time i'm unable to find that data.so find delta H and substitute it to equation..

2nd question also can be solved as same procedure...