Podcast
Questions and Answers
For a saturated NaCl solution, which process demonstrates the reversible nature of equilibrium?
For a saturated NaCl solution, which process demonstrates the reversible nature of equilibrium?
- Crystallizing and dissolving (correct)
- Crystal structure and bond energy
- Solidifying and melting
- Evaporating and condensing
In a system at equilibrium at varying conditions, what do the forward and reverse rates demonstrate?
In a system at equilibrium at varying conditions, what do the forward and reverse rates demonstrate?
- Forward rate increases, reverse rate remains constant
- Forward and reverse rates are independent of external conditions
- The relationship between forward and reverse reaction rates (correct)
- Rates are constantly changing in opposite directions
Based on a rate vs. time graph, how can you determine when equilibrium is reached?
Based on a rate vs. time graph, how can you determine when equilibrium is reached?
- The rate of the reverse reaction is zero
- The rate of the forward reaction is at its maximum
- The rate of the forward reaction is zero
- The rates of the forward and reverse reactions are equal (correct)
Consider the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ in a closed container. As the reaction approaches equilibrium, what happens to the rate of the reverse reaction?
Consider the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ in a closed container. As the reaction approaches equilibrium, what happens to the rate of the reverse reaction?
Consider the equilibrium: $H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)}$. If $H_2O$ and $CO$ are placed in a closed container at high temperature, what occurs as the system approaches equilibrium?
Consider the equilibrium: $H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)}$. If $H_2O$ and $CO$ are placed in a closed container at high temperature, what occurs as the system approaches equilibrium?
A 1.00 L flask contains a system at gaseous equilibrium. What is the immediate effect of adding more reactants to this flask?
A 1.00 L flask contains a system at gaseous equilibrium. What is the immediate effect of adding more reactants to this flask?
Consider the equilibrium: $2NH_{3(g)} \rightleftharpoons N_{2(g)} + 3H_{2(g)}$. If a flask is initially filled with $NH_3$, how does the rate of the forward reaction change as equilibrium is approached?
Consider the equilibrium: $2NH_{3(g)} \rightleftharpoons N_{2(g)} + 3H_{2(g)}$. If a flask is initially filled with $NH_3$, how does the rate of the forward reaction change as equilibrium is approached?
Consider the equilibrium: $N_2O_{4(g)} + heat \rightleftharpoons 2NO_{2(g)}$. If a 1.0 L container is initially filled with 2.0 mol of $NO_2$, how does the rate of reaction of $NO_2$ change as the system approaches equilibrium?
Consider the equilibrium: $N_2O_{4(g)} + heat \rightleftharpoons 2NO_{2(g)}$. If a 1.0 L container is initially filled with 2.0 mol of $NO_2$, how does the rate of reaction of $NO_2$ change as the system approaches equilibrium?
For the equilibrium $SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$, if a 1.0 L container is initially filled with 2.0 mol of $SO_2Cl_2$, how does the rate of the forward reaction change as the system approaches equilibrium?
For the equilibrium $SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$, if a 1.0 L container is initially filled with 2.0 mol of $SO_2Cl_2$, how does the rate of the forward reaction change as the system approaches equilibrium?
Consider the reversible reaction: $Fe^{3+}{(aq)} + SCN^-{(aq)} \rightleftharpoons FeSCN^{2+}_{(aq)}$. If $Fe(NO_3)_3$ is added to a solution of KSCN, how do the forward and reverse reaction rates change as the reaction proceeds?
Consider the reversible reaction: $Fe^{3+}{(aq)} + SCN^-{(aq)} \rightleftharpoons FeSCN^{2+}_{(aq)}$. If $Fe(NO_3)_3$ is added to a solution of KSCN, how do the forward and reverse reaction rates change as the reaction proceeds?
If equal moles of $N_2$ and $O_2$ are added to a closed container under certain conditions, how does the reverse reaction in the equilibrium $N_{2(g)} + 2O_{2(g)} \rightleftharpoons 2NO_{2(g)}$ change as the system approaches equilibrium?
If equal moles of $N_2$ and $O_2$ are added to a closed container under certain conditions, how does the reverse reaction in the equilibrium $N_{2(g)} + 2O_{2(g)} \rightleftharpoons 2NO_{2(g)}$ change as the system approaches equilibrium?
For the equilibrium $2O_{3(g)} \rightleftharpoons 3O_{2(g)}$ with $K_{eq} = 65$, if a 1.0L container initially contains 0.10 moles of $O_3$ and 0.10 moles of $O_2$, how will the concentrations change as the reaction proceeds towards equilibrium?
For the equilibrium $2O_{3(g)} \rightleftharpoons 3O_{2(g)}$ with $K_{eq} = 65$, if a 1.0L container initially contains 0.10 moles of $O_3$ and 0.10 moles of $O_2$, how will the concentrations change as the reaction proceeds towards equilibrium?
For the equilibrium $H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)}$, what happens to the concentrations of the reactants and products in a closed container initially filled with $H_2O$ and $CO$ as the system approaches equilibrium?
For the equilibrium $H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)}$, what happens to the concentrations of the reactants and products in a closed container initially filled with $H_2O$ and $CO$ as the system approaches equilibrium?
Which statement accurately describes all chemical equilibrium systems?
Which statement accurately describes all chemical equilibrium systems?
Which of the following applies to all systems at equilibrium?
Which of the following applies to all systems at equilibrium?
What is true in all systems at equilibrium?
What is true in all systems at equilibrium?
Consider the equilibrium: $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$. At equilibrium, how does the rate of decomposition of $SO_3$ relate to the rate of formation of $O_2$?
Consider the equilibrium: $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$. At equilibrium, how does the rate of decomposition of $SO_3$ relate to the rate of formation of $O_2$?
Which statement is true for all equilibrium systems?
Which statement is true for all equilibrium systems?
Which of the following is true for all systems at equilibrium?
Which of the following is true for all systems at equilibrium?
What is a characteristic of all systems at equilibrium?
What is a characteristic of all systems at equilibrium?
What must a system at equilibrium have?
What must a system at equilibrium have?
When do macroscopic properties become constant in an equilibrium system?
When do macroscopic properties become constant in an equilibrium system?
Which statement is NOT true for all chemical equilibrium systems?
Which statement is NOT true for all chemical equilibrium systems?
Which statement applies to a chemical equilibrium?
Which statement applies to a chemical equilibrium?
Chemical equilibrium is said to be dynamic because:
Chemical equilibrium is said to be dynamic because:
Equilibrium is considered a dynamic process because:
Equilibrium is considered a dynamic process because:
Equilibrium is said to be dynamic because:
Equilibrium is said to be dynamic because:
A system at equilibrium is said to be dynamic because at equilibrium:
A system at equilibrium is said to be dynamic because at equilibrium:
A chemical equilibrium is described as dynamic because:
A chemical equilibrium is described as dynamic because:
For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)} + energy$, what describes the changes in enthalpy and entropy as the reaction proceeds?
For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)} + energy$, what describes the changes in enthalpy and entropy as the reaction proceeds?
In which reaction is entropy decreasing?
In which reaction is entropy decreasing?
For the equilibrium $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 92 \text{ kJ}$, the forward reaction can be described as:
For the equilibrium $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 92 \text{ kJ}$, the forward reaction can be described as:
In which reaction is the enthalpy of the reactants greater than the enthalpy of the products?
In which reaction is the enthalpy of the reactants greater than the enthalpy of the products?
Consider $Na_2CO_{3(s)} + 2HCl_{(aq)} \rightarrow 2NaCl_{(aq)} + CO_{2(g)} + H_2O_{(l)}, \Delta H = -27.7 \text{ kJ}$. Which statement is true?
Consider $Na_2CO_{3(s)} + 2HCl_{(aq)} \rightarrow 2NaCl_{(aq)} + CO_{2(g)} + H_2O_{(l)}, \Delta H = -27.7 \text{ kJ}$. Which statement is true?
Consider $N_2O_{(g)} + NO_{2(g)} \rightarrow 3NO_{(g)}, \Delta H = +156 \text{ kJ}$. Which statement is correct?
Consider $N_2O_{(g)} + NO_{2(g)} \rightarrow 3NO_{(g)}, \Delta H = +156 \text{ kJ}$. Which statement is correct?
In which of the following does the entropy decrease?
In which of the following does the entropy decrease?
For which of the following systems will the factors of entropy and enthalpy both favor the reactants?
For which of the following systems will the factors of entropy and enthalpy both favor the reactants?
For the reaction $C_3H_{8(8)} + 5O_{2(g)} → 3CO_{2(8)} + 4H_2O_{(8)}, \Delta H = -2202 \text{ kJ}$, which of the following applies to the forward reaction?
For the reaction $C_3H_{8(8)} + 5O_{2(g)} → 3CO_{2(8)} + 4H_2O_{(8)}, \Delta H = -2202 \text{ kJ}$, which of the following applies to the forward reaction?
Which reaction results in an entropy increase?
Which reaction results in an entropy increase?
In an endothermic equilibrium system:
In an endothermic equilibrium system:
Chemical systems tend to move towards positions of:
Chemical systems tend to move towards positions of:
Consider $C_2H_{2(g)} + H_{2(g)} \rightleftharpoons C_2H_{4(g)}$ with $\Delta H = -175 \text{ kJ}$. Which statement regarding enthalpy and entropy is correct?
Consider $C_2H_{2(g)} + H_{2(g)} \rightleftharpoons C_2H_{4(g)}$ with $\Delta H = -175 \text{ kJ}$. Which statement regarding enthalpy and entropy is correct?
In which of the following reactions do the minimum enthalpy and maximum entropy oppose each other?
In which of the following reactions do the minimum enthalpy and maximum entropy oppose each other?
Which of the following systems would the tendencies toward minimum enthalpy and maximum entropy be in opposition to each other?
Which of the following systems would the tendencies toward minimum enthalpy and maximum entropy be in opposition to each other?
In which of the following do both minimum enthalpy and maximum entropy favor the reactants?
In which of the following do both minimum enthalpy and maximum entropy favor the reactants?
Flashcards
Dynamic Equilibrium
Dynamic Equilibrium
A system where the forward and reverse reactions occur at equal rates, resulting in no net change in reactant and product concentrations.
Le Chatelier's Principle
Le Chatelier's Principle
A principle stating that if a change of condition is applied to a system in equilibrium, the system will shift in a direction that relieves the stress.
Equilibrium Constant (Keq)
Equilibrium Constant (Keq)
The ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to the power of its stoichiometric coefficient.
Chemical Equilibrium Systems
Chemical Equilibrium Systems
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Macroscopic properties become constant in an equilibrium system when
Macroscopic properties become constant in an equilibrium system when
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Equilibrium
Equilibrium
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Dynamic
Dynamic
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Enthalpy in Equilibrium
Enthalpy in Equilibrium
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Entropy in Equilibrium
Entropy in Equilibrium
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Increased Pressure
Increased Pressure
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Decreased Temperature
Decreased Temperature
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Equilibrium shifts to right.
Equilibrium shifts to right.
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Value change
Value change
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High Value
High Value
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Sets
Sets
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Increases the amount of moles
Increases the amount of moles
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Shift that adds the catalyst
Shift that adds the catalyst
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Increased pressure
Increased pressure
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Equilibrium is achieved sooner
Equilibrium is achieved sooner
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Equilibrium will shift
Equilibrium will shift
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Addition catalyst.
Addition catalyst.
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Increase volume catalyst
Increase volume catalyst
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If temp decreases.
If temp decreases.
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Keq
Keq
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Increased of volume
Increased of volume
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Endothermic reaction
Endothermic reaction
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A low percentage
A low percentage
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The products side
The products side
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High temperature
High temperature
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NO4
NO4
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Study Notes
Dynamic Equilibrium Study Guide Overview
- The study guide contains questions from provincial exams since April 1994
- Questions are similar from year to year
- Identification of question types helps efficiently answer questions on the provincial exam
Recommendations for Using the Study Guide
- Practice ALL questions in the booklet
- Attempt the questions before consulting the answer key to maximize learning
- Figure out why you are wrong, talk with a study partner, get together with a group to work through them
- Get 100% on any Chemistry 12 multiple choice test
- Avoid marking answers on the questions themselves to reuse the study guide effectively
- Indicate questions wrong with an asterisk or note to revisit them
- Use a check mark of assurance of understanding
- Check off STATUS box on the PRESCRIBED LEARNING OUTCOMES sheet for familiarity with the material
Introduction to Dynamic Equilibrium
- Saturated NaCl(aq) solution exemplifies equilibrium due to the reversible nature of crystallizing and dissolving
- The relationship between forward and reverse reaction rates in an equilibrium system can be represented graphically
- At equilibrium, the rate of the forward reaction can be determined from a graph
- As nitrogen and oxygen gases react in a closed container towards equilibrium, the rate of the reverse reaction increases as concentration of products increase
- For H2O and CO placed in a closed container and approaching system equilibrium, the rate of the forward reaction increases and the rate of the reverse reaction decreases
- Adding reactants to a gaseous equilibrium system in a 1.00 L flask results in a shift to the right and an increase products concentration
- In a flask initially filled with NH3, the rate of the forward reaction decreases as the system approaches equilibrium, while the rate of the reverse reaction increases
- With N2O4(g) + heat 2NO2(g) equilibrium and initially filling a 1.0 L container with 2.0 mol of NO2, as the system approaches equilibrium, the rate of reaction of NO2 decreases and [N2O4] increases
- In SO2Cl2(g) ⇄ SO2(g) + Cl2(g) equilibrium and initially with a 1.0 L container filled with 2.0 mol of SO2Cl2, as the reaction proceeds towards equilibrium, the rate of the forward reaction decreases and the [SO2] decreases
- In Fe3+(aq) + SCN-(aq) ⇄ FeSCN2+(aq) equilibrium, the addition of Fe(NO3)3 to KSCN solution causes an increase in rates of forward reaction and reverse reaction as the reaction moves towards equilibrium
- For N2(g) + 2O2(g) ⇄ 2NO2(g), adding equal moles of N2 and O2 to a closed container increases the rate of the reverse reaction and increases [NO2] as the system proceeds toward equilibrium
- With 2O3(g) ⇄ 3O2(g) equilibrium, increasing [O3] and increasing [O2] happens as the reaction proceeds towards equilibrium
- In H2O(g) + CO(g) ⇄ H2(g) + CO2(g) equilibrium, filling a closed container initially with H2O and CO results in [CO] decreasing and [CO2] increasing as the reaction proceeds towards equilibrium
- The rate of the forward reaction equals the rate of the reverse reaction describing all chemical equilibrium systems
- Equal forward and reverse rates and constant macroscopic properties apply to all equilibrium systems
- In all systems at equilibrium the concentration of reactants and the concentration of products are constant
- At equilibrium, the rate of decomposition of SO3 equals the rate of formation of SO3 for 2SO3(g) 2SO2(g) + O2(g)
- The equilibrium can be achieved from either products or reactants, macroscopic properties is constant for all equilibrium systems
- Rate of the forward reaction equals the rate of the reverse reaction for all equilibrium systems
- Two opposing reactions occur at the same rate characterize all systems at equilibrium
- A system at equilibrium must have constant temperature, equal rates of forward and reverse reactions
- Macroscopic properties become constant in an equilibrium system when forward and reverse reaction rates are equal
- Equal concentrations of reactants and products does not apply to all chemical equilibrium systems
- Forward and reverse reaction rates are equal, equilibrium can be achieved from either direction, macroscopic properties are constant applies to a chemical equilibrium
- Chemical equilibrium is dynamic because both forward and reverse reactions are occurring
- Equilibrium is a dynamic process because forward and reverse reactions continue to occur
- Equilibrium dynamic because the forward and reverse reactions continue
- Chemical equilibrium is dynamic because both reactants and products continue to form
Enthalpy and Entropy
- In N2(g) + 3H2(g) → 2NH3(g) + energy, as the reaction proceeds, enthalpy decreases and entropy decreases
- Entropy decreases in Fe3+ (aq)+ SCN-(aq) → FeSCN2+(aq)
- Forward reaction in N2(g) + 3H2(g) ⇄ 2NH3(g) + 92 kJ is exothermic and entropy is decreasing
- The enthalpy of the reactants is greater than the enthalpy of the products in H2O(s) → H2O(l)
- In Na2CO3(s) + 2HCl(aq) → 2NaCl(aq) + CO2(g) + H2O(l), minimum enthalpy and maximum entropy both favour products
- For N2O(g) + NO2(g) → 3NO(g), the minimum enthalpy and maximum entropy both favor the reactants
- For 2NO2(g) ⇄ N2O4(g) + 59 kJ, both minimum enthalpy and maximum entropy favor reactants
- In 2NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g), entropy decreases
- Reactants will be favored by the factors of entropy and enthalpy in 3C(s) + 3H2(g) + heat ⇄ C3H6(g)
- The reaction 2C(s) + O2(g) → 2CO(g) results in an entropy increase
- In an endothermic equilibrium system, minimum enthalpy and maximum entropy both favour products
- Chemical systems tend to move toward positions of minimum enthalpy and maximum entropy
- Given C2H2(g) + H2(g) ⇄ C2H4(g), the system reaches equilibrium because the enthalpy factor favours the product and the entropy factor favours the reactants
- The tendency towards minimum enthalpy and maximum entropy oppose each other in N2(g) + O2(g) → NO2(g)
- The tendencies toward minimum enthalpy and maximum entropy are in opposition to each other in 2C(g) + 2H2(g) → C2H4(g)
Le Chatelier's Principle
-
In 4NH3(g) + 5O2(g) ⇄ 4NO(g) + 6H2O(g) + energy, the equilibrium will shift to the left by adding H2O(g)
-
The equilibrium shifts to the right, and Keg remains constant when the volume of the container is increased
-
In 2SO2(g) + O2(g)⇄ 2SO3(g) + energy, the equilibrium will shift to the left by increasing the volume
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The equilibrium will shift to the left in 2NO(g) + Br2(g) + energy ⇄ 2NOBr(g) by increasing the temperature
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When the temperature is increased, the equilibrium shifts to the right for with N2(g) + O2(g) + energy ⇄ 2NO(g)
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2NO2(g) ⇄ N2O4(g) + energy equilibrium will shift removing some N2O4
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The addition of H2 will cause the equilibrium to shift to the right and [CH4] will increase in C(s) + 2H2(g) ⇄ CH4(g)
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The equilibrium concentration of PCl5 will increase when Cl2 is removed in PCl5(g) ⇄ PCl3(g) + Cl2(g)
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The equilibrium does not shift and [N2O4] increases if the volume is decreased
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Decreasing the volume will result in decreasing the mass of NH4CI with NH3(g) + HCI(g) ⇄ NH4CI(s) + energy
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The concentrations of all species remain constant as comparing the new equilibrium with the original equilibrium when pressure is increased by reducing the volume
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Addition of a catalyst occurs at time t1
-
Adding HNO3 will decrease [CrO42-] from 2CrO42-(aq) + 2H+(aq) ⇄ Cr2O72-(aq) + H2O(l)
-
The equilibrium doesn't shift with a change in volume, temperature, concentration of products, concentration of reactants if SO2(g) + NO2(g) ⇄ SO3(g) + NO(g) + energy
-
When the temperature is decreased, the equilibrium shifts left and [SO2Cl2] increases in SO2Cl2(g) + energy ⇄ SO2(g) + Cl2(g)
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The equilibrium shifts right in the volume of the system is increased when decreasing the system for equilibrium with N2O4(g) + 58 kJ ⇄ 2NO2(g)
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In equilibrium with CH₄(g) + H₂O(g) + heat ⇄ CO(g) + 3H₂(g), increase in temperature alongside an increased volume will shift the equilibrium to the right
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Given the equilibrium with 2HI(g) ⇄ H2(g) + I2(g) ΔH = −68 kJ, decreasing the temperature causes the equilibrium to shift right
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The equilibrium will shift to the to the right of the additions with 2SO2(g) + O2(g) ⇄ 2SO3(g)
-
The equilibrium shift to the left if adding I2
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The equilibrium always shifts to favour the endothermic when the temperature is increased
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A decrease in volume and a decrease in temperature will shift the equilibrium to 2NH3(g) + 92 kJ
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Increasing temperature while the system has constant volume, a new state of equilibrium is established where is an increase in [CO] and an increase in Keg
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The volume of the system is decreased at a constant temperature. A new state of equilibrium is established by a shift of the original equilibrium to the left with [SO3] increases
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Adding B. H₂O will increase [OH] from equilibrium, to system with = NH3(aq) + H₂O(l) ⇄ NH4(aq) + OH(aq)
-
When a small amount of solid C is added to the system of C(s)+2H2(g) ⇄ CH4(g) + 74 kJ , all concentrations remain constant
-
[H2 and [CO] will net decrease in systems from following added CO2/H2/CO/H2O as reaction proceeds toward equilibrium, the ⇄ CO(g)+H2O(g)
-
decreasing the volume, would have no impact, and Hydrogen(H2) will remain constant if equilibrium position of [H3] , In has a slight increase of the of system with + 10 is then increased and is set on this position and how system?
-
Decreasing the volume to shift system in CaCO3 (s) CaO (s) + CO2 (g) [ the pressure has 16+ in which, a. would on that shifts that for which temperature/when? 284 with . [N2O4 has, added in with the volume decreases, B would
- . , on that of that as with an temperature, A left B The shifts which, Cl2(g), PCl3(g), is/volume
-
[SO2CI2] to shifted 9 . . : , of (2) what value in temperature 166 67, by
volume
-
some has volume' that, [1200 2(3) in. on decrease (decreases), rate/increases. A1 for to 003+ if be, shifts, C decreases if of .5: the . SAHOTA
Reaction Rates
- Adding SO2 increased the rate, reverse and forward as the system approaches equilibrium
- Increasing temperature the rates increases -Temperature has the systems in immediate and which rate on effect 2 decreases the
- Equilibrium will endothermically and decreases then, shift increases forward by equilibrium if of the of rates constant, increase of product product of yield decrease the then for (Keq) then how the catalyst, system
Equilibrium Constant
- There will be Nno shift in this equilibrium when a catalyst is added
- Which of the following will
- the system is then SAHOTA will and. A shift when catalyst equilibrium added with B equilibrium and rate (89 (90 , equilibrium D to increased
-
Equilibrium D is the the HCL
-
. with, on system increase The (NH3)0 2(g) the volume the as The volume -47 2:
,
Equilibrium Constants:
The most product favored equilibrium in terms of K 2 55 is2 to one-step
- 2: 2 in product in on which large has -0, if reactant has constant to . : if to is: the then A that . The 222 (Cl,2(g)+3H The Cl , then :The 1 [HI D. if is the . Then 4] The system A: the equilibrium in by SAHO
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