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Predict whether adding potassium nitrate impacts the solubility of ammonium nitrate. NH4NO3(s) ⇌ NH4+ (aq) + NO3-(aq)
Predict whether adding potassium nitrate impacts the solubility of ammonium nitrate. NH4NO3(s) ⇌ NH4+ (aq) + NO3-(aq)
The correct mathematical expression for finding the molar solubility (S) of Sn(OH)2 is:
The correct mathematical expression for finding the molar solubility (S) of Sn(OH)2 is:
The molar solubility of AgCl (Ksp = 1.6 × 10⁻¹⁰) in 0.0034 M sodium chloride at 25°C is:
The molar solubility of AgCl (Ksp = 1.6 × 10⁻¹⁰) in 0.0034 M sodium chloride at 25°C is:
Which of the following processes is spontaneous under the specified conditions?
Which of the following processes is spontaneous under the specified conditions?
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A certain process has ΔSuniv > 0 at 25°C. What does one know about the process?
A certain process has ΔSuniv > 0 at 25°C. What does one know about the process?
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Which of the following is always true for an exothermic process?
Which of the following is always true for an exothermic process?
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For a reaction in a voltaic cell, both ΔH° and ΔS° are positive. Which of the following statements is true?
For a reaction in a voltaic cell, both ΔH° and ΔS° are positive. Which of the following statements is true?
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The heat of vaporization for 1.0 mole of water at 100°C and 1.0 atm is 40.56 kJ/mol. Calculate ΔS for the process H2O(l) → H2O(g) at 100°C.
The heat of vaporization for 1.0 mole of water at 100°C and 1.0 atm is 40.56 kJ/mol. Calculate ΔS for the process H2O(l) → H2O(g) at 100°C.
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The standard free energy of formation of AgI(s) is –66.2 kJ/mol. What is ΔG° for the reaction 2AgI(s) → 2Ag(s) + I2(s)?
The standard free energy of formation of AgI(s) is –66.2 kJ/mol. What is ΔG° for the reaction 2AgI(s) → 2Ag(s) + I2(s)?
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Given: CH3COOH(aq) ⇌ H+(aq) + CH3COO–(aq) Ka = 1.75 × 10⁻⁵ at 25°C. What is ΔG at 25°C for the solution?
Given: CH3COOH(aq) ⇌ H+(aq) + CH3COO–(aq) Ka = 1.75 × 10⁻⁵ at 25°C. What is ΔG at 25°C for the solution?
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Select all that apply. Place a check for all processes that involve an increase in the entropy of the system.
Select all that apply. Place a check for all processes that involve an increase in the entropy of the system.
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For each pair, which species has the higher entropy? Write it in the space provided, followed by explain why it is higher. a. Mg(NO₃)₂(s), Mg(NO₃)₂(aq)
For each pair, which species has the higher entropy? Write it in the space provided, followed by explain why it is higher. a. Mg(NO₃)₂(s), Mg(NO₃)₂(aq)
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What is the oxidation state for the nitrogen atom in HNO3?
What is the oxidation state for the nitrogen atom in HNO3?
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What is the oxidation state for the nitrogen atom in NO2?
What is the oxidation state for the nitrogen atom in NO2?
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What is the oxidation state for the nitrogen atom in N2O?
What is the oxidation state for the nitrogen atom in N2O?
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What is the oxidation state for nitrogen in NH4Cl?
What is the oxidation state for nitrogen in NH4Cl?
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What is the oxidation state for nitrogen in NaNO2?
What is the oxidation state for nitrogen in NaNO2?
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In the reaction 2Ca(s) + O2(g) → 2CaO(s), which species is oxidized?
In the reaction 2Ca(s) + O2(g) → 2CaO(s), which species is oxidized?
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In the reaction 2Cs(s) + Cl2(g) → 2CsCl(s), Cl2 is:
In the reaction 2Cs(s) + Cl2(g) → 2CsCl(s), Cl2 is:
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In the reaction N2(g) + 3H2(g) → 2NH3(g), N2 is:
In the reaction N2(g) + 3H2(g) → 2NH3(g), N2 is:
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Given the reaction: 2MnO4– + 5H2O2 + 6H+ → 2Mn2+ + 8H2O + 5O2, determine the number of electrons involved in this reaction.
Given the reaction: 2MnO4– + 5H2O2 + 6H+ → 2Mn2+ + 8H2O + 5O2, determine the number of electrons involved in this reaction.
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Which of the following are oxidation-reduction reactions? I. PCl3 + Cl2 → PCl5 II. Cu + 2AgNO3 → Cu(NO3)2 + 2Ag III. CO2 + 2LiOH → Li2CO3 + H2O IV. FeCl2 + 2NaOH → Fe(OH)2 + 2NaCl
Which of the following are oxidation-reduction reactions? I. PCl3 + Cl2 → PCl5 II. Cu + 2AgNO3 → Cu(NO3)2 + 2Ag III. CO2 + 2LiOH → Li2CO3 + H2O IV. FeCl2 + 2NaOH → Fe(OH)2 + 2NaCl
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Study Notes
Constants
- R = 8.3145 J/(K·mol)
- R = 0.08206 L·atm/(K·mol)
Equations
- ΔSsurr = –ΔH/T
- ΔG = ΔH - TΔS
- ΔG° = -RT lnK
- ΔG° = ΔH° - TΔS°
- ΔG = ΔG° + RT lnQ
Solution Equilibria
- Effects of adding a common ion on solubility:
- Adding potassium nitrate to a solution of ammonium nitrate may affect its solubility
- Molar solubility (S) of Sn(OH)2:
- Expression: 2S2 = Ksp
- Factors affecting solubility:
- Presence of common ions
- Concentration of ions
Thermochemistry
- Spontaneity of processes:
- ΔSsurr > 0 indicates a spontaneous process
- Exothermic and endothermic processes:
- Exothermic: ΔSsurr < 0, q sys < 0
- Endothermic: ΔSsurr > 0, q sys > 0
- Relation between ΔG° and E°cell:
- E°cell will increase with an increase in temperature if ΔS° is positive
- Standard free energy of formation (ΔG°f):
- Example: ΔG°f for AgI(s) is -66.2 kJ/mol
Thermodynamics
- Entropy (S):
- Increases with increase in disorder or randomness
- Example: mixing 5 mL ethanol with 25 mL water increases entropy
- Thermodynamic parameters:
- ΔSsystem: positive for increase in entropy
- ΔHsystem: positive for endothermic, negative for exothermic
- ΔSsurrounding: opposite of ΔSsystem
- ΔG: negative for spontaneous, positive for non-spontaneous
- ΔSuniverse: always increases
Electrochemistry
- Oxidation and reduction:
- Oxidation: loss of electrons
- Reduction: gain of electrons
- Examples of oxidation-reduction reactions:
- 2Ca(s) + O2(g) → 2CaO(s)
- 2Cs(s) + Cl2(g) → 2CsCl(s)
- Identifying oxidizing and reducing agents:
- Oxidizing agent: O2 in 2Ca(s) + O2(g) → 2CaO(s)
- Reducing agent: Ca in 2Ca(s) + O2(g) → 2CaO(s)
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Description
Practice quiz for Chem 101B Chapter 15, covering solution equilibria and related equations and constants. Test your knowledge on thermodynamic properties and chemical reactions.
