1) Rank the reactions from fastest to slowest. a) 1, 2, 3, 4, 5 b) 5, 4, 3, 2, 1 c) 3, (1, 2, & 4), 5 d) 5, (1, 2, & 4), 3 2) Which of the reactions are exothermic? (select all that apply) a) 1 b) 2 c) 3 d) 4 e) 5 3) Which of the following involve an increase in the entropy of the system? a) melting of a solid b) sublimation c) freezing d) mixing e) separation f) boiling 4) Given the values of ∆H and ∆S, which of the following changes will be spontaneous at constant temperature & pressure? a) ∆H = +25 kJ, ∆S = +5.0 J/K, T = 300 K b) ∆H = +25 kJ, ∆S = +100 J/K, T = 300 K c) ∆H = -10 kJ, ∆S = +5.0 J/K, T = 298 K d) ∆H = -10 kJ, ∆S = -40 J/K, T = 200 K 5) For ammonia (NH3), the enthalpy of fusion is 5.65 kJ/mol and the entropy of fusion is 28.9 J/K∙mol. Will NH3(s) spontaneously melt at 200 K? a) yes (∆G is negative) b) yes (∆G is positive) c) no (∆G is negative) d) no (∆G is positive) 6) For ammonia (NH3), the enthalpy of fusion is 5.65 kJ/mol and the entropy of fusion is 28.9 J/K∙mol. What is the approximate melting point of ammonia?  a) 196 K b) 298 K c) 310 K d) 137 K e) 0.196 K f) 5 K 7) Predict the sign of ∆S for the change shown. Assume all of the equations are balanced. a) positive b) negative c) no change d) cannot be determined 8) Predict the sign of ∆S for the change shown. Assume all of the equations are balanced.  a) positive b) negative c) no change d) cannot be determined 9) Predict the sign of ∆S for the change shown. Assume all of the equations are balanced.  a) positive b) negative c) no change d) cannot be determined 10) Predict the sign of ∆Sℴ for the change shown. Assume all of the equations are balanced.  a) positive b) negative c) no change d) cannot be determined 11) Calculate ∆Gℴ for CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) a) -919 kJ b) 29 kJ c) -817 kJ d) -131 kJ 12) 2NO2(g)⇌ N2O4(g) The values of ∆Hℴ and ∆Sℴ are -58.03 kJ/mol and -176.6 J/K∙mol, respectively.  Calculate the value of K at 25.0℃.  a) -5.403 b) 5.403 c) 1.002 d) 3.090 e) 2.743 f) 0.055 13) Calculate ∆Gℴ for H2O(g) + ½O2(g) ⇌ H2O2(g) at 600. K.  a) 100 kJ b) 141 kJ c) 173 kJ d) 245 kJ e) 372 kJ f) 902 kJ

Thermodynamics Review

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