Podcast
Questions and Answers
The forward reaction of PCl3 and Cl2 producing PCl~5 is ______.
The forward reaction of PCl3 and Cl2 producing PCl~5 is ______.
exothermic
Introducing more PCl~3 into the mixture will shift the equilibrium to the ______.
Introducing more PCl~3 into the mixture will shift the equilibrium to the ______.
right
Increasing pressure will favor the side with the ______ number of molecules.
Increasing pressure will favor the side with the ______ number of molecules.
smaller
If the temperature is increased, the equilibrium will shift in the ______ direction.
If the temperature is increased, the equilibrium will shift in the ______ direction.
The reaction between iron (III) chloride and potassium thiocyanate forms a ______ complex.
The reaction between iron (III) chloride and potassium thiocyanate forms a ______ complex.
Adding hydrochloric acid caused the red color to ______ as the equilibrium shifted.
Adding hydrochloric acid caused the red color to ______ as the equilibrium shifted.
When potassium thiocyanate is added to the second tube, the red complex ______.
When potassium thiocyanate is added to the second tube, the red complex ______.
Chemical equilibrium is a state of dynamic balance in a reversible reaction where the rate of the forward reaction is the same as the rate of the ______ reaction.
Chemical equilibrium is a state of dynamic balance in a reversible reaction where the rate of the forward reaction is the same as the rate of the ______ reaction.
Ammonia is one of the most important chemicals manufactured by the ______.
Ammonia is one of the most important chemicals manufactured by the ______.
A reversible reaction is one in which the products react to give back the ______, meaning the reaction can go in both directions.
A reversible reaction is one in which the products react to give back the ______, meaning the reaction can go in both directions.
Le Chatelier's Principle states that if a ______ is applied to a system at equilibrium, the system re-adjusts to relieve the stress applied.
Le Chatelier's Principle states that if a ______ is applied to a system at equilibrium, the system re-adjusts to relieve the stress applied.
An increase in pressure will favour the reaction that brings about a reduction in ______, shifting towards the side with the smaller number of molecules.
An increase in pressure will favour the reaction that brings about a reduction in ______, shifting towards the side with the smaller number of molecules.
In the forward reaction of 2NO2(g) to N2O4(g), heat is given out, making it an ______ reaction.
In the forward reaction of 2NO2(g) to N2O4(g), heat is given out, making it an ______ reaction.
A change in pressure affects only an equilibrium reaction that has unequal numbers of gaseous ______ and products.
A change in pressure affects only an equilibrium reaction that has unequal numbers of gaseous ______ and products.
ΔH with a negative sign indicates that a reaction has given out ______.
ΔH with a negative sign indicates that a reaction has given out ______.
A catalyst speeds up the rate at which ______ is reached but does not change the position of equilibrium.
A catalyst speeds up the rate at which ______ is reached but does not change the position of equilibrium.
Ammonia is manufactured by reacting nitrogen with ______
Ammonia is manufactured by reacting nitrogen with ______
A pressure of approximately ______ atmospheres is used in the production of Ammonia
A pressure of approximately ______ atmospheres is used in the production of Ammonia
The Haber process to maximize the yield of ammonia favors high ______ and low temperature
The Haber process to maximize the yield of ammonia favors high ______ and low temperature
Sulfuric Acid is manufactured by a process known as the ______ Process
Sulfuric Acid is manufactured by a process known as the ______ Process
The equilibrium constant, Kc, represents the relationship between the concentrations of the ______ and products
The equilibrium constant, Kc, represents the relationship between the concentrations of the ______ and products
The products in the equilibrium constant expression are always written ______ the line
The products in the equilibrium constant expression are always written ______ the line
A temperature of ______°C is the best temperature for the catalyst to work at in the Contact Process
A temperature of ______°C is the best temperature for the catalyst to work at in the Contact Process
In the equilibrium expression, each species concentration is raised to the power of its ______ in the balanced equation
In the equilibrium expression, each species concentration is raised to the power of its ______ in the balanced equation
When a yellow solution of iron(III) chloride (FeCl3) and a colourless solution of potassium thiocyanate (KCNS) were mixed, a ______ colour appeared.
When a yellow solution of iron(III) chloride (FeCl3) and a colourless solution of potassium thiocyanate (KCNS) were mixed, a ______ colour appeared.
The equilibrium constant (Kc) for the reaction was calculated to be ______.
The equilibrium constant (Kc) for the reaction was calculated to be ______.
Changing the ______ has no effect on this equilibrium as it is an equilibrium in solution with no gases involved.
Changing the ______ has no effect on this equilibrium as it is an equilibrium in solution with no gases involved.
The red colour faded when the test tube containing the equilibrium mixture was placed in an ______-water bath.
The red colour faded when the test tube containing the equilibrium mixture was placed in an ______-water bath.
The addition of KCNS caused the concentration of Fe^3+^ ions to ______ as the reaction shifted forward.
The addition of KCNS caused the concentration of Fe^3+^ ions to ______ as the reaction shifted forward.
The equilibrium constant expression for the reaction is ______ = [$\frac{{[NH}{3}]^{2}}{{[N}{2][H}_{2}]^{3}}$]
The equilibrium constant expression for the reaction is ______ = [$\frac{{[NH}{3}]^{2}}{{[N}{2][H}_{2}]^{3}}$]
At a certain high temperature T, the equilibrium constant (Kc) value for the reaction is equal to [$______$]
At a certain high temperature T, the equilibrium constant (Kc) value for the reaction is equal to [$______$]
Le Châtelier's principle states that if a system at equilibrium is subjected to a ______, it tends to oppose the stress.
Le Châtelier's principle states that if a system at equilibrium is subjected to a ______, it tends to oppose the stress.
Increases in temperature cause the value of Kc to ______ for an exothermic reaction.
Increases in temperature cause the value of Kc to ______ for an exothermic reaction.
The metals used as catalysts in catalytic converters include ______, palladium, and rhodium.
The metals used as catalysts in catalytic converters include ______, palladium, and rhodium.
Catalysis that occurs in catalytic converters is known as ______ catalysis.
Catalysis that occurs in catalytic converters is known as ______ catalysis.
One way that catalysts increase the rate of reaction is by lowering the ______.
One way that catalysts increase the rate of reaction is by lowering the ______.
A substance that could 'poison' the catalysts of the catalytic converter is ______ compounds.
A substance that could 'poison' the catalysts of the catalytic converter is ______ compounds.
Flashcards
Chemical Equilibrium
Chemical Equilibrium
A state of balance in a reversible reaction where the forward and backward reaction rates are equal.
Reversible Reaction
Reversible Reaction
A reaction that can proceed in both directions, forming products from reactants and vice-versa.
Le Chatelier's Principle
Le Chatelier's Principle
If a stress is applied to a system at equilibrium, the system will shift to relieve the stress.
Stress (in equilibrium)
Stress (in equilibrium)
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Effect of Pressure Change (gases)
Effect of Pressure Change (gases)
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Catalyst
Catalyst
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Exothermic Reaction
Exothermic Reaction
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Endothermic Reaction
Endothermic Reaction
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Effect of adding PCl3 on PCl5 concentration
Effect of adding PCl3 on PCl5 concentration
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Effect of increased pressure on PCl5 concentration
Effect of increased pressure on PCl5 concentration
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Effect of increased temperature on PCl5 concentration
Effect of increased temperature on PCl5 concentration
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Equilibrium shift (Fe3+ + SCN- ⇌ Fe(SCN)2+)
Equilibrium shift (Fe3+ + SCN- ⇌ Fe(SCN)2+)
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Haber Process
Haber Process
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Equilibrium Constant (Kc)
Equilibrium Constant (Kc)
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Dynamic Equilibrium
Dynamic Equilibrium
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Effect of Temperature on Kc
Effect of Temperature on Kc
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Effect of Pressure on Kc
Effect of Pressure on Kc
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Catalytic Converters
Catalytic Converters
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Heterogeneous Catalysis
Heterogeneous Catalysis
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Ammonia Production
Ammonia Production
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Haber Process Conditions
Haber Process Conditions
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Equilibrium Constant (Kc)
Equilibrium Constant (Kc)
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Equilibrium Constant Equation
Equilibrium Constant Equation
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Sulfuric Acid Production
Sulfuric Acid Production
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Contact Process Conditions
Contact Process Conditions
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Kc Calculation
Kc Calculation
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Effect of Adding Reactant
Effect of Adding Reactant
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Effect of Temperature
Effect of Temperature
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Study Notes
Chemical Equilibrium
- Definition: Chemical equilibrium is a dynamic state in a reversible reaction where the forward and backward reaction rates are equal.
- Reversible Reaction: A reaction where products can react to reform reactants.
- Dynamic State: Reactants continuously form products, and products continuously form reactants.
- Le Chatelier's Principle: If a stress is applied to a system at equilibrium, the system will shift to relieve the stress.
- Stress: Changes in reaction conditions (concentration, pressure, temperature).
Le Chatelier's Principle Examples
- Concentration: Increasing reactant concentration shifts equilibrium toward product formation. Decreasing product concentration has the same effect.
- Pressure: Increasing pressure favors the side with fewer gas molecules. Decreasing pressure favors the side with more gas molecules.
- Temperature: Endothermic reactions shift toward products with increased temperature. Exothermic reactions shift toward products with decreased temperature. The sign of ΔH indicated whether the reaction is exothermic (+ΔH) or endothermic (-ΔH).
Effect of Change of Pressure in Gaseous Reactions
- Increasing pressure in a gaseous reaction shifts equilibrium toward the side with fewer gaseous molecules.
- A change in pressure affects only reactions with unequal numbers of gaseous reactants and products.
- The fewer gaseous molecules occupy less volume and help to relieve the pressure.
Equilibrium Constant (Kc)
- Definition: Kc is a constant that represents the relationship between the concentrations of reactants and products at equilibrium.
- The concentrations of products are written above the line, and reactants below the line.
- Each species' concentration is raised to the power of its coefficient in the balanced equation,
- K_c = [C]c[D]d / [A]a[B]b. (C and D are products, A and B are reactants)
Industrial Applications
- Ammonia Production (Haber Process): High pressure and low temperature favor ammonia production.
- Sulfuric Acid Production (Contact Process): Optimized temperature (450°C) and pressure to maximize sulfur trioxide production.
Exam Questions
- Equilibrium Constant Expression: The expression defines the relationship of the equilibrium constant (e.g., Kp) with the concentrations of products and reactants at a given temperature.
- Equilibrium Calculation: Equilibrium calculations (e.g., finding equilibrium concentrations or moles of reactants and products) involve using the equilibrium constant expression to find unknown concentrations.
Le Chatelier's Principle – Additional Points
- Effect of Temperature: Temperature changes affect the value of Kc.
- Catalysts: Catalysts increase the rate of reaction but do not change the position of equilibrium.
- Equilibrium Position: The equilibrium position represents the ratio of product to reactant concentrations at equilibrium.
- Dynamic nature of Equilibrium: A reversible chemical reaction in which the rate of the forward reaction is equal to the rate of the backward reaction.
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Description
This quiz covers the concepts of chemical equilibrium, including its definitions, reversible reactions, and the dynamic state of reactions. Additionally, it explores Le Chatelier's Principle, illustrating how changes in concentration, pressure, and temperature affect equilibrium. Test your understanding of these fundamental chemistry principles.
