5) Predict the direction of the entropy change in each of the following reactions (i.e. write either INCREASE or DECREASE in the blank space at the end of the statement). a) CaCO3(s) → CaO(s) + CO2(g) b) NH3(g) + HCl(g) → NH4Cl(s) c) 2NaHCO3(s) → Na₂CO3(s) + H₂O(g) + CO2(g) d) CaO (s) + CO2(g) → CaCO3(s)

For each of the following reactions determine if the change in entropy was positive or negative:A) Water at 40°C → Water at 25°CB) 2NO2(g) → N2O4(g)C) CH3OH (l) → CH3OH (g)D) PbCl2(s) → PbCl2(aq)

What is the change in entropy, AS, for the following reaction? Use Table G in your book for values of standard entropies. Your answer should be in J/K mol. CaCO3(s) + 2 H'(aq) → → Ca² (aq) + H₂O(l) + CO2(g) O 264.9 J/K mol O 118.6 J/K mol 394.3 J/K mol 137.7 J/K mol 2

Using enthalpies of formation, calculate deltaH for the following reaction at 25°C. Also calculate deltaS for this reaction from standard entropies at 25°C. Use these values to calculate deltaG for the reaction at this temperature. Species  deltaHf(kJ/mol)  S(J/mol⋅K) CH3OH(l) –238.7 126.8 O2(g) 0 205.0 CO2(g) –393.5 213.7 H2O(l) –285.8 69.95 2CH3OH(l) +3O2(g) --- 2CO2(g) + 4H2O(l) deltaH =  kJ deltaS =  J/K deltaG =  kJ

Use the data to calculate the standard entropy change for the following reaction: 5. S°[Mt(s)] 43.2 J/K mol Mt(s) + ½ O2(g) → MtO(s) S°[O2(g)] = 305.1 J/K-mol S°[MtO(s)] 62.6 J/K mol a) -133.2 J/K b) -285.7 J/K c) 285.7 J/K d) 133.2 J/K

AG (ky/mol) SUbStance / 1on so (ky/mol) -1206.9 /moi k) 92.9 • CaC03l>) -|128.8 • CaO (s) |- 635. I – 60 3.5 38.2 • CO2(9) - 393.5 - 394.4 213.7 191.5 3 H2(g) 202.7 ZNH3 ) -45.9 -16 193 • Hz (g) 202.7 223.0 -92.31 - 95. 30 186.79

list any physical changes you can think of in which entropy increases (ΔS = +)