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Questions and Answers
What is the primary reason for not using high pressures in some industrial reactions?
Which of the following describes why chemical equilibrium is considered dynamic?
In the expression for Kc, what is placed in the numerator?
How does an increase in temperature affect a chemical equilibrium that is exothermic?
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What is the effect of decreasing pressure on a gaseous equilibrium?
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What occurs when a reactant is added to a system at equilibrium?
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Which temperature is deemed ideal for the Haber process?
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What catalyst is used in the contact process?
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What color change indicates that an equilibrium shift has occurred when potassium thiocyanate is added?
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What conclusion can be drawn about the endothermic reaction based on temperature changes observed in the experiment?
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Study Notes
Industrial Reactions and High Pressures
- High pressures can pose danger, notably increasing the risk of explosions in industrial settings.
Dynamic Nature of Chemical Equilibrium
- Chemical equilibrium is dynamic as it involves continual formation and consumption of products and reactants.
Expression for Equilibrium Constant (Kc)
- Kc is determined by the ratio of the concentrations of products raised to their stoichiometric coefficients over the concentrations of reactants raised to their stoichiometric coefficients.
Temperature Effects on Equilibrium
- Increasing temperature favors endothermic reactions, which absorb heat to restore balance.
- Decreasing temperature favors exothermic reactions, which release heat energy to counteract the loss of heat.
Pressure Effects on Equilibrium
- An increase in pressure shifts equilibrium towards the side with fewer gaseous moles, reducing overall gas volume.
- A decrease in pressure shifts equilibrium towards the side with more gaseous moles, increasing gas volume.
Changes in Concentration and Equilibrium
- Adding a reactant shifts equilibrium towards the opposite side to utilize the added substance.
- Removing a substance shifts equilibrium towards the side where the substance is depleted to replenish it.
Ideal Conditions for the Haber Process
- Optimal conditions for ammonia production: low temperature, high pressure (500°C and 250 atm).
Ideal Conditions for the Contact Process
- Suitable conditions: low temperature and high pressure, typically 450°C and above atmospheric pressure.
Challenges with Low Temperatures
- Operating at too low a temperature is uneconomical due to insufficient reaction rates for production.
Catalyst in the Contact Process
- Vanadium pentoxide serves as the catalyst for the conversion of sulfur dioxide to sulfur trioxide.
Le Chatelier’s Principle Experiment
- The experiment involves the equilibrium reaction: Fe³⁺ + CNS⁻ ⇌ Fe(CNS)²⁺.
Concentration Changes in the Experiment
- Adding HCl reduces Fe³⁺ concentration, causing the solution to turn yellow; adding potassium thiocyanate shifts equilibrium right, turning the solution red.
Temperature Changes in the Experiment
- A test tube placed in a hot water bath becomes yellow; cold water bath results in a more intense red, indicating temperature influence on equilibrium.
Conclusion from Color Changes
- The observed color shifts during temperature changes suggest that the reaction is endothermic, as heat absorption leads to the formation of products.
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Description
This quiz explores key concepts of chemical equilibrium, including the dynamics of equilibrium reactions and the impacts of temperature on reaction kinetics. You'll also learn about the expression for Kc and the practical considerations of using high pressures in industrial processes.
