For the reactions corresponding to the fifth digit of your Student ID Number, find ΔG° at 50 °C and at 90 °C. Does the spontaneity increase or decrease as the temperature increases?
Set 0)
Solid strontium chloride reacting with aqueous carbonate ion.
Aqueous nitric acid reacting with solid calcium hydroxide.
Aqueous bicarbonate ion reacting with aqueous cyanide ion.
Set 1)
Solid magnesium chloride reacting with aqueous carbonate ion.
Aqueous nitric acid reacting with solid barium hydroxide.
Aqueous bicarbonate ion reacting with aqueous cyanide ion.
Set 2)
Solid calcium chloride reacting with aqueous carbonate ion.
Aqueous nitric acid reacting with solid zinc(II) hydroxide.
Aqueous bicarbonate ion reacting with aqueous cyanide ion.
Set 3)
Solid barium chloride reacting with aqueous carbonate ion.
Aqueous nitric acid reacting with solid nickel(II) hydroxide.
Aqueous bicarbonate ion reacting with aqueous cyanide ion.
Set 4)
Solid iron(II) chloride reacting with aqueous carbonate ion.
Aqueous nitric acid reacting with solid magnesium hydroxide.
Aqueous bicarbonate ion reacting with aqueous cyanide ion.
Set 5)
Solid silver nitrate reacting with aqueous sulfate ion.
Aqueous sulfuric acid reacting with solid sodium hydroxide.
Aqueous bicarbonate ion reacting with aqueous cyanide ion.
Set 6)
Solid silver nitrate reacting with aqueous chloride ion.
Aqueous sulfuric acid reacting with solid potassium hydroxide.
Aqueous bicarbonate ion reacting with aqueous cyanide ion.
Set 7)
Solid silver nitrate reacting with aqueous bromide ion.
Aqueous sulfuric acid reacting with aqueous sodium hydroxide.
Aqueous bicarbonate ion reacting with aqueous cyanide ion.
Set 8)
Solid silver nitrate reacting with aqueous iodide ion.
Aqueous sulfuric acid reacting with aqueous potassium hydroxide.
Aqueous bicarbonate ion reacting with aqueous cyanide ion.
Set 9)
Solid silver nitrate reacting with aqueous sulfide ion.
Aqueous sulfuric acid reacting with solid lithium hydroxide.
Aqueous bicarbonate ion reacting with aqueous cyanide ion.
ΔH° is taken from Homework 23
ΔS° is taken from Homework 24
Set 0)
SrCl2(s) + CO32–(aq) → SrCO3(s) + 2 Cl–(aq)
ΔH° = –47 kJ/mole
ΔS° = +150. J/mole·K
ΔG° (50 °C) = (–47) – (323)(0.150) = –95. kJ/mole
ΔG° (90 °C) = (–47) – (363)(0.150) = –101. kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
2 HNO3(aq) + Ca(OH)2(s) → 2 H2O(l) + Ca2+(aq) + 2 NO3–(aq)
ΔH° = –123.7 kJ/mole
ΔS° = +1.2 J/mole·K
ΔG° (50 °C) = (–123.7) – (323)(0.0012) = –124.1 kJ/mole
ΔG° (90 °C) = (–123.7) – (363)(0.0012) = –124.1 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
HCO3–(aq) + CN–(aq) → ← HCN(aq) + CO32–(aq)
ΔH° = –32 kJ/mole
ΔS° = –141 J/mole·K
ΔG° (50 °C) = (–32) – (323)(–0.141) = +14. kJ/mole
ΔG° (90 °C) = (–32) – (363)(–0.141) = +19. kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
Set 1)
MgCl2(s) + CO32–(aq) → MgCO3(s) + 2 Cl–(aq)
ΔH° = –112 kJ/mole
ΔS° = +146.0 J/mole·K
ΔG° (50 °C) = (–112) – (323)(0.1460) = –159. kJ/mole
ΔG° (90 °C) = (–112) – (363)(0.1460) = –165. kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
2 HNO3(aq) + Ba(OH)2(s) → 2 H2O(l) + Ba2+(aq) + 2 NO3–(aq)
ΔH° = –158.4 kJ/mole
ΔS° = +42. J/mole·K
ΔG° (50 °C) = (–158.4) – (323)(0.042) = –172.0 kJ/mole
ΔG° (90 °C) = (–158.4) – (363)(0.042) = –173.6 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
HCO3–(aq) + CN–(aq) → ← HCN(aq) + CO32–(aq)
ΔH° = –32 kJ/mole
ΔS° = –141 J/mole·K
ΔG° (50 °C) = (–32) – (323)(–0.141) = +14. kJ/mole
ΔG° (90 °C) = (–32) – (363)(–0.141) = +19. kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
Set 2)
CaCl2(s) + CO32–(aq) → CaCO3(s) + 2 Cl–(aq)
ΔH° = –69 kJ/mole
ΔS° = +154 J/mole·K
ΔG° (50 °C) = (–69) – (323)(0.154) = –119. kJ/mole
ΔG° (90 °C) = (–69) – (363)(0.154) = –125. kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
2 HNO3(aq) + Zn(OH)2(s)→2 H2O(l) + Zn2+(aq) + 2 NO3–(aq)
ΔH° = –78.8 kJ/mole
ΔS° = –53.5 J/mole·K
ΔG° (50 °C) = (–78.8) – (323)(–0.0535) = –61.5 kJ/mole
ΔG° (90 °C) = (–78.8) – (363)(–0.0535) = –59.4 kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
HCO3–(aq) + CN–(aq) → ← HCN(aq) + CO32–(aq)
ΔH° = –32 kJ/mole
ΔS° = –141 J/mole·K
ΔG° (50 °C) = (–32) – (323)(–0.141) = +14. kJ/mole
ΔG° (90 °C) = (–32) – (363)(–0.141) = +19. kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
Set 3)
BaCl2(s) + CO32–(aq) → BaCO3(s) + 2 Cl–(aq)
ΔH° = –15 kJ/mole
ΔS° = +158. J/mole·K
ΔG° (50 °C) = (–15) – (323)(0.158) = –66. kJ/mole
ΔG° (90 °C) = (–15) – (363)(0.158) = –72. kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
2 HNO3(aq) + Ni(OH)2(s) → 2 H2O(l) + Ni2+(aq) + 2 NO3–(aq)
ΔH° = –101.1 kJ/mole
ΔS° = –107. J/mole·K
ΔG° (50 °C) = (–101.1) – (323)(–0.107) = –66.5 kJ/mole
ΔG° (90 °C) = (–101.1) – (363)(–0.107) = –62.3 kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
HCO3–(aq) + CN–(aq) → ← HCN(aq) + CO32–(aq)
ΔH° = –32 kJ/mole
ΔS° = –141 J/mole·K
ΔG° (50 °C) = (–32) – (323)(–0.141) = +14. kJ/mole
ΔG° (90 °C) = (–32) – (363)(–0.141) = +19. kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
Set 4)
FeCl2(s) + CO32–(aq) → FeCO3(s) + 2 Cl–(aq)
ΔH° –56.1 kJ/mole
ΔS° = 144.8 J/mole·K
ΔG° (50 °C) = (–56.1) – (323)(0.1448) = –102.9 kJ/mole
ΔG° (90 °C) = (–56.1) – (363)(0.1448) = –108.7 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
2 HNO3(aq) + Mg(OH)2(s) → 2 H2O(l) + Mg2+(aq) + 2 NO3–(aq)
ΔH° = –109.0 kJ/mole
ΔS° = –61.5 J/mole·K
ΔG° (50 °C) = (–109.0) – (323)(–0.0615) = –89.1 kJ/mole
ΔG° (90 °C) = (–109.0) – (363)(–0.0615) = –86.7 kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
HCO3–(aq) + CN–(aq) → ← HCN(aq) + CO3(aq)
ΔH° = –32 kJ/mole
ΔS° = –141 J/mole·K
ΔG° (50 °C) = (–32) – (323)(–0.141) = +14. kJ/mole
ΔG° (90 °C) = (–32) – (363)(–0.141) = +19. kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
Set 5)
2 AgNO3(s) + SO42–(aq) → Ag2SO4(s) + 2 NO3–(aq)
ΔH° = +32.2 kJ/mole
ΔS° = +191.3 J/mole·K
ΔG° (50 °C) = (32.2) – (323)(0.1913) = –29.6 kJ/mole
ΔG° (90 °C) = (32.2) – (363)(0.1913) = –37.2 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
H2SO4(aq) + 2 NaOH(s) → 2 H2O(l) + 2 Na+(aq) + SO42–(aq)
ΔH° = –200.6 kJ/mole
ΔS° = +128.9 J/mole·K
ΔG° (50 °C) = (–200.6) – (323)(0.1289) = –242.2 kJ/mole
ΔG° (90 °C) = (–200.6) – (363)(0.1289) = –247.4 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
HCO3–(aq) + CN–(aq) → ← HCN(aq) + CO3(aq)
ΔH° = –32 kJ/mole
ΔS° = –141 J/mole·K
ΔG° (50 °C) = (–32) – (323)(–0.141) = +14. kJ/mole
ΔG° (90 °C) = (–32) – (363)(–0.141) = +19. kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
Set 6)
AgNO3(s) + Cl–(aq) → AgCl(s) + NO3–(aq)
ΔH° = –40.5 kJ/mole
ΔS° = +45.2 J/mole·K
ΔG° (50 °C) = (–40.5) – (323)(0.0452) = –55.2 kJ/mole
ΔG° (90 °C) = (–40.5) – (363)(0.0452) = –56.9 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
H2SO4(aq) + 2 KOH(s) → 2 H2O(l) + 2 K+(aq) + SO42–(aq)
ΔH° = –226.8 kJ/mole
ΔS° = +187.1 J/mole·K
ΔG° (50 °C) = (–226.8) – (323)(0.1871) = –287.2 kJ/mole
ΔG° (90 °C) = (–226.8) – (363)(0.1871) = –294.7 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
HCO3–(aq) + CN–(aq) → ← HCN(aq) + CO3(aq)
ΔH° = –32 kJ/mole
ΔS° = –141 J/mole·K
ΔG° (50 °C) = (–32) – (323)(–0.141) = +14. kJ/mole
ΔG° (90 °C) = (–32) – (363)(–0.141) = +19. kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
Set 7)
AgNO3(s) + Br–(aq) → AgBr(s) + NO3–(aq)
ΔH° = –60.1 kJ/mole
ΔS° = +32 J/mole·K
ΔG° (50 °C) = (–60.1) – (323)(0.032) = –70.4 kJ/mole
ΔG° (90 °C) = (–60.1) – (363)(0.032) = –71.7 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
H2SO4(aq) + 2 NaOH(aq) → 2 H2O(l) + 2 Na+(aq) + SO42–(aq)
ΔH° = –113.4 kJ/mole
ΔS° = +161.6 J/mole·K
ΔG° (50 °C) = (–113.4) – (323)(0.1616) = –165.6 kJ/mole
ΔG° (90 °C) = (–113.4) – (363)(0.1616) = –172.1 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
HCO3–(aq) + CN–(aq) → ← HCN(aq) + CO3(aq)
ΔH° = –32 kJ/mole
ΔS° = –141 J/mole·K
ΔG° (50 °C) = (–32) – (323)(–0.141) = +14. kJ/mole
ΔG° (90 °C) = (–32) – (363)(–0.141) = +19. kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
Set 8)
AgNO3(s) + I–(aq) → AgI(s) + NO3–(aq)
ΔH° = –87.3 kJ/mole
ΔS° = +9 J/mole·K
ΔG° (50 °C) = (–87.3) – (323)(0.009) = –90.2 kJ/mole
ΔG° (90 °C) = (–87.3) – (363)(0.009) = –90.6 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
H2SO4(aq) + 2 KOH(aq) → 2 H2O(l) + 2 K+(aq) + SO42–(aq)
ΔH° = –111.6 kJ/mole
ΔS° = +161.6 J/mole·K
ΔG° (50 °C) = (–111.6) – (323)(0.1616) = –163.8 kJ/mole
ΔG° (90 °C) = (–111.6) – (363)(0.1616) = –170.3 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
HCO3–(aq) + CN–(aq) → ← HCN(aq) + CO3(aq)
ΔH° = –32 kJ/mole
ΔS° = –141 J/mole·K
ΔG° (50 °C) = (–32) – (323)(–0.141) = +14. kJ/mole
ΔG° (90 °C) = (–32) – (363)(–0.141) = +19. kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
Set 9)
2 AgNO3(s) + S2–(aq) → Ag2S(s) + 2 NO3–(aq)
ΔH° = –234.8 kJ/mole
ΔS° = +135 J/mole·K
ΔG° (50 °C) = (–234.8) – (323)(0.135) = –278.4 kJ/mole
ΔG° (90 °C) = (–234.8) – (363)(0.135) = –283.8 kJ/mole
Spontaneity increases with increasing temperature because ΔG° becomes more negative.
H2SO4(aq) + 2 LiOH(s) → 2 H2O(l) + 2 Li+(aq) + SO42–(aq)
ΔH° = –158.8 kJ/mole
ΔS° = –13.4 J/mole·K
ΔG° (50 °C) = (–158.8) – (323)(–0.0134) = –154.5 kJ/mole
ΔG° (90 °C) = (–158.8) – (363)(–0.0134) = –153.9 kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.
HCO3–(aq) + CN–(aq) → ← HCN(aq) + CO3(aq)
ΔH° = –32 kJ/mole
ΔS° = –141 J/mole·K
ΔG° (50 °C) = (–32) – (323)(–0.141) = +14. kJ/mole
ΔG° (90 °C) = (–32) – (363)(–0.141) = +19. kJ/mole
Spontaneity decreases with increasing temperature because ΔG° becomes more positive.