Podcast
Questions and Answers
Which of the following is true about colligative properties?
Which of the following is true about colligative properties?
- The relative number of solute molecules and the nature of the solute and the solvent affect colligative properties
- The relative number of solute molecules in the solution and nature of the solvent affect colligative properties (correct)
- The relative number of solvent molecules affect colligative properties
- The relative number of solute molecules is irrespective of the solute and the solvent nature
According to Raoult’s law, what does the relative lowering of saturated vapour pressure depend on for a dilute solution?
According to Raoult’s law, what does the relative lowering of saturated vapour pressure depend on for a dilute solution?
- The relative lowering of saturated vapour pressure is equal to the mole fraction of the solute (correct)
- The relative lowering of saturated vapour pressure is proportional to the amount of the solute in the solution
- The lowering of saturated vapour pressure is equal to the mole fraction of the solute
- The saturated vapour pressure of the solution is equal to the mole fraction of the solvent
What does the vapour pressure of the solvent above the solution depend on?
What does the vapour pressure of the solvent above the solution depend on?
- Molar concentration of the solvent
- Mole fraction of the solute
- Molar concentration of the solute
- Mole fraction of the solvent (correct)
Which statement correctly describes the freezing point of the solution (Tf)?
Which statement correctly describes the freezing point of the solution (Tf)?
Which of the following best describes the boiling point of a solution?
Which of the following best describes the boiling point of a solution?
What determines the osmotic pressure of a solution?
What determines the osmotic pressure of a solution?
What is the characteristic of Kb (the molar boiling point elevation constant)?
What is the characteristic of Kb (the molar boiling point elevation constant)?
What happens to osmotic pressure when the temperature decreases?
What happens to osmotic pressure when the temperature decreases?
What type of solution has a lower osmotic pressure than a reference solution?
What type of solution has a lower osmotic pressure than a reference solution?
Which solution has the higher osmotic pressure among the options?
Which solution has the higher osmotic pressure among the options?
What is the osmotic pressure of a 0.1 M nonelectrolyte solution at 0°C?
What is the osmotic pressure of a 0.1 M nonelectrolyte solution at 0°C?
Which statement is correct for Vant Hoff’s law?
Which statement is correct for Vant Hoff’s law?
Which expressions are used for determination of molar concentration?
Which expressions are used for determination of molar concentration?
What is correct for determination of a molar mass of a substance?
What is correct for determination of a molar mass of a substance?
What is the boiling point (Tb) of a 1M glucose solution?
What is the boiling point (Tb) of a 1M glucose solution?
What is the freezing point (Tf) of a 1M glucose solution?
What is the freezing point (Tf) of a 1M glucose solution?
Which statement about ionic strength is correct?
Which statement about ionic strength is correct?
Which species has the highest activity factor for K+ ions?
Which species has the highest activity factor for K+ ions?
According to Lewis concept, which statement is true about acids?
According to Lewis concept, which statement is true about acids?
Which statement regarding Ostwald's dilution law is correct?
Which statement regarding Ostwald's dilution law is correct?
Among the given equimolar solutions, which one has the lowest ionic strength?
Among the given equimolar solutions, which one has the lowest ionic strength?
Which statement about the activity factor of NO3 - ions is correct?
Which statement about the activity factor of NO3 - ions is correct?
Which compound has the highest ionic strength among ZnSO4, Na2SO4, and NaCl?
Which compound has the highest ionic strength among ZnSO4, Na2SO4, and NaCl?
According to Bronsted-Lowry concept, what happens to the conjugate base as the acid gets stronger?
According to Bronsted-Lowry concept, what happens to the conjugate base as the acid gets stronger?
Which solvents have a leveling effect on acids?
Which solvents have a leveling effect on acids?
Which equation is used to determine the ionic strength for strong electrolytes?
Which equation is used to determine the ionic strength for strong electrolytes?
Which type of system does not allow transfer of matter but allows transfer of energy to and from surroundings?
Which type of system does not allow transfer of matter but allows transfer of energy to and from surroundings?
Which of the following is an example of a state function?
Which of the following is an example of a state function?
What is the equation for entropy change (ΔS) in terms of the entropy change of the system (ΔSsys) and the entropy change of the surroundings (ΔSsurr)?
What is the equation for entropy change (ΔS) in terms of the entropy change of the system (ΔSsys) and the entropy change of the surroundings (ΔSsurr)?
What is the criteria for spontaneity of a reaction?
What is the criteria for spontaneity of a reaction?
Which thermodynamic potential measures the maximum reversible work that can be done by a system at constant temperature and pressure?
Which thermodynamic potential measures the maximum reversible work that can be done by a system at constant temperature and pressure?
What is the equation for Gibbs free energy change (ΔG) for a reaction?
What is the equation for Gibbs free energy change (ΔG) for a reaction?
For which type of reaction does the heat released have a negative value?
For which type of reaction does the heat released have a negative value?
What type of reaction absorbs energy from its surroundings?
What type of reaction absorbs energy from its surroundings?
Which law deals with the relationship between heat changes that occur during a series of reactions?
Which law deals with the relationship between heat changes that occur during a series of reactions?
What does the change in Gibbs free energy (ΔG) for a reaction represent?
What does the change in Gibbs free energy (ΔG) for a reaction represent?
What quantity is independent of the path taken to reach that state?
What quantity is independent of the path taken to reach that state?
What potential measures the disorder or randomness of a system?
What potential measures the disorder or randomness of a system?
Which of the following factors does NOT affect the dissociation constant (K) of a weak electrolyte?
Which of the following factors does NOT affect the dissociation constant (K) of a weak electrolyte?
Which of the following statements about the dissociation degree of a weak electrolyte (α) is correct?
Which of the following statements about the dissociation degree of a weak electrolyte (α) is correct?
When NH4Cl is added to a solution of NH4OH, what happens to the concentration of OH–?
When NH4Cl is added to a solution of NH4OH, what happens to the concentration of OH–?
Which factor does NOT practically affect the dissociation degree of acetic acid in an aqueous solution?
Which factor does NOT practically affect the dissociation degree of acetic acid in an aqueous solution?
Which equation is correct for polyprotic acids?
Which equation is correct for polyprotic acids?
Which expressions are correct for the relationship between Ka, Kb, and Kw?
Which expressions are correct for the relationship between Ka, Kb, and Kw?
Which expressions are correct for Kw, [H+], and [OH–]?
Which expressions are correct for Kw, [H+], and [OH–]?
If Ka for an acid is 10–5, what is the pKb value of its conjugate base?
If Ka for an acid is 10–5, what is the pKb value of its conjugate base?
If pKa values of four acids at 25°C are given below, what is the pKa of the strongest acid?
If pKa values of four acids at 25°C are given below, what is the pKa of the strongest acid?
[OH–] ion concentration in a solution is 10^–4, what is the pH of the solution?
[OH–] ion concentration in a solution is 10^–4, what is the pH of the solution?
If the pH of a solution is 4 and it increases up to 5, what should be the change in the H+ ion concentration?
If the pH of a solution is 4 and it increases up to 5, what should be the change in the H+ ion concentration?
What is the equation for calculating pH of a weak acid solution?
What is the equation for calculating pH of a weak acid solution?
What type of system allows transfer of neither matter nor energy to and from its surroundings?
What type of system allows transfer of neither matter nor energy to and from its surroundings?
Which of the following is an example of a closed system?
Which of the following is an example of a closed system?
Which type of system is the human body an example of?
Which type of system is the human body an example of?
Which of the following are state functions?
Which of the following are state functions?
What is a thermodynamic state function?
What is a thermodynamic state function?
Which of the following is not a state function?
Which of the following is not a state function?
According to Hess's law, the thermal effects of a reaction depend on...
According to Hess's law, the thermal effects of a reaction depend on...
Enthalpy changes of a reaction depend on...
Enthalpy changes of a reaction depend on...
The enthalpy change of a reaction does not depend on the...
The enthalpy change of a reaction does not depend on the...
The enthalpies of the elements in their standard states are...
The enthalpies of the elements in their standard states are...
The enthalpy of formation of a compound from the elements ...
The enthalpy of formation of a compound from the elements ...
The heat of neutralization is constant when dilute solution of...
The heat of neutralization is constant when dilute solution of...
Which of the following neutralization reactions have the highest neutralization heat?
Which of the following neutralization reactions have the highest neutralization heat?
Which of the following is NOT correct?
Which of the following is NOT correct?
When ice melts into water, entropy…
When ice melts into water, entropy…
Which of the following expressions is correct?
Which of the following expressions is correct?
What happens to the concentration of OH– when NH4Cl is added to a solution of NH4OH?
What happens to the concentration of OH– when NH4Cl is added to a solution of NH4OH?
Study Notes
- A closed system is a system where transfer of matter is not possible, but transfer of energy to and from surroundings ispossible.
- Examples of closed systems: some amount of hot water enclosed in a closed container.
- Human body is an example of an open system, as it exchanges matter with the environment.
- State functions are thermodynamic potentials that only depend on the current state of a system and not on the path taken to reach that state.
- Examples of state functions: internal energy (ΔE), entropy (S), and enthalpy (H).
- A thermodynamic state function is a quantity whose value is independent of the path taken to reach that state.
- Heat of compound formation is the heat absorbed or released when one mole of a compound is formed from its elements in their standard states.
- Enthalpy changes of a reaction depend on the conditions of the reaction, initial and final concentration, and the physical state of reactants and products.
- For an exothermic reaction, the heat released is a negative value.
- Entropy is a measure of disorder and increases when a system undergoes a spontaneous change.
- The Gibbs free energy (G) is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
- An endothermic reaction is a reaction that absorbs energy from its surroundings, and for it to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
- The criteria for spontaneity of a reaction: ΔG < 0.
- Gibbs free energy, enthalpy, and entropy are related through the legacy of Gibbs, specifically through the equation G = H - TS.
- Gibbs free energy is the maximum reversible work that can be done by a system at constant temperature and pressure.
- For an endothermic reaction to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
- Internal energy (ΔE) is a state function that measures the maximum reversible work that can be done by a system at constant temperature and volume.
- Enthalpy (H) is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
- Entropy (S) is a thermodynamic potential that measures the disorder or randomness of a system.
- Hess's law deals with the relationship between heat changes that occur during a series of reactions.
- The thermal effects of a reaction depend on the initial and final conditions of the reacting substances.
- Enthalpy changes of a reaction are independent of the number of intermediate steps involved in the reaction.
- Heat of compound formation is the heat absorbed or released when one mole of a compound is formed from its elements in their standard states.
- The enthalpy change of a reaction is the difference in enthalpy between the reactants and the products.
- The heat of neutralization is the heat absorbed or released when an acid and a base react to form a salt and water.
- The heat of neutralization is constant for dilute solutions of strong acids and strong bases.
- When ice melts, the entropy increases due to the increase in the number of translationally disordered water molecules.
- The equation for entropy change (ΔS) in terms of the entropy change of the system (ΔSsys) and the entropy change of the surroundings (ΔSsurr) is: ΔS = ΔSsys + ΔSsurr > 0.
- The Gibbs free energy change (ΔG) for a reaction is given by the equation: ΔG = ΔH - TΔS.
- For a spontaneous reaction, ΔG is negative, which means that the enthalpy change is less than the product of the temperature (T) and entropy change (ΔS) of the reaction.
- The criteria for spontaneity of a reaction are: ΔG < 0.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The change in Gibbs free energy (ΔG) for a reaction is given by the equation: ΔG = ΔH - TΔS.
- For a reaction to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
- The Gibbs free energy change (ΔG) is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
- The change in Gibbs free energy (ΔG) for a reaction is the difference between the enthalpy change (ΔH) and the product of the temperature (T) and entropy change (ΔS) of the reaction.
- For an endothermic reaction to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
- The Gibbs free energy change (ΔG) is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for an endothermic reaction to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
- The Gibbs free energy change (ΔG) for a reaction is given by the equation: ΔG = ΔH - TΔS.
- For an endothermic reaction to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
- The change in Gibbs free energy (ΔG) for a reaction is the difference between the enthalpy change (ΔH) and the product of the temperature (T) and entropy change (ΔS) of the reaction.
- The Gibbs free energy change (ΔG) is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
- The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work
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Test your knowledge of weak electrolyte dissociation with this quiz. Answer questions about factors affecting dissociation constant (K) and the dissociation degree (α) of weak electrolytes.