Calculate the standard enthalpy of reaction, Δ?∘rxn,, of each of the given acid–base neutralization reactions involving the strong base KOH. The standard enthalpy of formation data are provided. Compound or Ion Standard Enthalpy of Formation (kJ/mol) KOH(aq) −482.4 H2O(l) −285.8 HClO3(aq) −98.4 KClO3(aq) −349.5 HBr(aq) −121.0 KBr(aq) −372.1 NH+4(aq) −132.5 NH3(aq) −80.3 K+(aq) −251.2 HClO3(aq)+KOH(aq)⟶KClO3(aq)+H2O(l) Δ?∘rxn=_________________kJ/mol HBr(aq)+KOH(aq)⟶KBr(aq)+H2O(l) Δ?∘rxn=__________________kJ/mol NH+4(aq)+KOH(aq)⟶NH3(aq)+K+(aq)+H2O(l) Δ?∘rxn=_________________kJ/mol Based on the Δ?∘rxn values, what is the most likely conclusion about the strength of the acids? 1. HClO3(aq) and HBr(aq) are weak acids, and NH+4(aq) is a strong acid. 2. HClO3(aq), HBr(aq), and NH+4(aq) are all strong acids. 3. HClO3(aq), HBr(aq), and NH+4(aq) are all weak acids. 4. HClO3(aq) and HBr(aq) are strong acids, and NH+4(aq) is a weak acid.
Calculate the standard enthalpy of reaction, Δ?∘rxn,, of each of the given acid–base neutralization reactions involving the strong base KOH. The standard enthalpy of formation data are provided.
|
Compound or Ion |
Standard Enthalpy of Formation (kJ/mol) |
|
KOH(aq) |
−482.4 |
|
H2O(l) |
−285.8 |
|
HClO3(aq) |
−98.4 |
|
KClO3(aq) |
−349.5 |
|
HBr(aq) |
−121.0 |
|
KBr(aq) |
−372.1 |
|
NH+4(aq) |
−132.5 |
|
NH3(aq) |
−80.3 |
|
K+(aq) |
−251.2 |
HClO3(aq)+KOH(aq)⟶KClO3(aq)+H2O(l)
Δ?∘rxn=_________________kJ/mol
HBr(aq)+KOH(aq)⟶KBr(aq)+H2O(l)
Δ?∘rxn=__________________kJ/mol
NH+4(aq)+KOH(aq)⟶NH3(aq)+K+(aq)+H2O(l)
Δ?∘rxn=_________________kJ/mol
Based on the Δ?∘rxn values, what is the most likely conclusion about the strength of the acids?
1. HClO3(aq) and HBr(aq) are weak acids, and NH+4(aq) is a strong acid.
2. HClO3(aq), HBr(aq), and NH+4(aq) are all strong acids.
3. HClO3(aq), HBr(aq), and NH+4(aq) are all weak acids.
4. HClO3(aq) and HBr(aq) are strong acids, and NH+4(aq) is a weak acid.
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