5. For each of the solution processes below, calculate ∆S o soln, given the values of S o given: i) C6H14O(l) −−→ C6H14O(aq), S o C6H14O(l) = 288.7 J K-1 mol-1 , S o C6H14O(aq) = 245.2 J K-1 mol-1 ii) C3H8O(l) −−→ C3H8O(aq), S o C3H8O(l) = 193.0 J K-1 mol-1 , S o C3H8O(aq) = 170.7 J K-1 mol-1 iii) C2H6 (g) −−→ C2H6 (aq), S o C2H6 (g) = 229.2 J K-1 mol-1 , S o C2H6 (aq) = 112.0 J K-1 mol-1 iv) KBr(s) −−→ KBr(aq), S o KBr(s) = 95.9 J K-1 mol-1 , S o KBr(aq) = 184.9 J K-1 mol-1

asked by @tamaraw6 • 11 months ago • Chemistry • 5 pts

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Hey there Tamara! So for each of these reactions we want to calculate their ΔS of reaction.

You will use this formula: ΔSrxn= sum of S of the products - sum of S of the reactants.

i) ΔS= [245.2 J/K mol] - [288.7 J/K mol] = -43.5 J/K

Do this for all the reactions. Note that in each reaction you have 1 mole of each reactant and product. If you had different number of moles for each, you would have to multiply the S values given by the number of moles of each, because those values are only per 1 mole.

Hope this helps! Let us know if you have any more questions.

answered by @dashab2 • 11 months ago