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Questions and Answers
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)
- Solubility does not change
- Solubility decreases (correct)
- Solubility increases
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:
- 8S3 = Ksp
- 2S3 = Ksp
- 4S3 = Ksp
- 2S2 = Ksp (correct)
- 108S5 = Ksp
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:
- 1.6 × 10⁻¹⁰
- 5.4 × 10⁻¹³
- 4.7 × 10⁻⁸ (correct)
- 0.0034
- none of these
Which of the following processes is spontaneous under the specified conditions?
Which of the following processes is spontaneous under the specified conditions?
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?
Which of the following is always true for an exothermic process?
Which of the following is always true for an exothermic process?
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?
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.
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)?
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?
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.
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)
What is the oxidation state for the nitrogen atom in HNO3?
What is the oxidation state for the nitrogen atom in HNO3?
What is the oxidation state for the nitrogen atom in NO2?
What is the oxidation state for the nitrogen atom in NO2?
What is the oxidation state for the nitrogen atom in N2O?
What is the oxidation state for the nitrogen atom in N2O?
What is the oxidation state for nitrogen in NH4Cl?
What is the oxidation state for nitrogen in NH4Cl?
What is the oxidation state for nitrogen in NaNO2?
What is the oxidation state for nitrogen in NaNO2?
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?
In the reaction 2Cs(s) + Cl2(g) → 2CsCl(s), Cl2 is:
In the reaction 2Cs(s) + Cl2(g) → 2CsCl(s), Cl2 is:
In the reaction N2(g) + 3H2(g) → 2NH3(g), N2 is:
In the reaction N2(g) + 3H2(g) → 2NH3(g), N2 is:
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.
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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