Chemical EquilibriaFlashcards - AQA Chemistry

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Do you need to solve quadratic equations to calculate the equilibrium amounts in this example?

No, this example has been carefully set up to avoid the formation of a quadratic equation.

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"Do you need to solve quadratic equations to calculate the equilibrium amounts in this example?"	"No, this example has been carefully set up to avoid the formation of a quadratic equation."
"What happens to the position of equilibrium and the value of K if the temperature is increased in this exothermic reaction?"	"The position of equilibrium shifts left and the value of K gets smaller."
"Describe the effect of pressure on the position of equilibrium in this equilibrium with fewer moles of gas on the product side."	"The position of equilibrium shifts right."
"Do catalysts have any effect on the value of K or the position of equilibrium in this reaction?"	"No, catalysts have no effect on the value of K or the position of equilibrium."
"Describe how to calculate the amounts of each component in an equilibrium mixture using the value of K."	"By setting up an equation using the stoichiometry of the reaction and the equilibrium constant, K, and solving for the unknown variable."
"What is the equation used to calculate the equilibrium amounts of each substance in a reaction?"	"(0.2 - x) / V = K"
"Define equimolar reaction."	"An equimolar reaction is a reaction where the number of moles of reactants is equal to the number of moles of products."
"How can the volume, V, be canceled out in the equation for calculating equilibrium amounts?"	"Since the reaction is equimolar, the volume, V, can be canceled out."
"Describe the experiment to work out the equilibrium constant Kc for an esterification reaction."	"Mixing ethanol, ethanoic acid, and a sulphuric acid catalyst in a boiling tube, allowing it to reach equilibrium for one week, and then titrating the mixture with sodium hydroxide."
"What is the purpose of using a sulphuric acid catalyst in the esterification reaction?"	"To increase the rate of the reaction."
"How can the initial amount of moles of reactants be calculated in the esterification experiment?"	"By using the densities and volumes of the liquids added."
"Describe the process of titrating the equilibrium mixture in the esterification experiment."	"Transferring a portion of the equilibrium mixture to a conical flask, adding phenolphthalein indicator, and titrating it with sodium hydroxide until the mixture turns pink."
"Describe how to calculate the equilibrium amount of ethanol at equilibrium."	"The equilibrium amount of ethanol can be calculated by subtracting the amount of ethanol that reacted from the initial amount of ethanol."
"Define the equilibrium constant (K) in terms of the concentrations of ethanol, ethyl ethanoate, ethanoic acid, and water."	"The equilibrium constant (K) is defined as the ratio of the concentrations of ethyl ethanoate and water to the concentrations of ethanoic acid and ethanol."
"How can you determine if one week is sufficient time for equilibrium to be established in a mixture?"	"To determine if one week is sufficient, you can make several mixtures and leave them for different amounts of time. If the resulting equilibrium constant (K) is the same value, it can be concluded that the time is sufficient."
"Describe the process of calculating the equilibrium amount of ethyl ethanoate at equilibrium."	"The equilibrium amount of ethyl ethanoate can be calculated by adding the amount that formed to the initial amount of ethyl ethanoate."
"Explain the Haber process for the production of ammonia."	"The Haber process involves the reaction of nitrogen and hydrogen gases at high temperature and pressure in the presence of an iron catalyst. This reaction produces ammonia, which is used in the production of fertilizers and other chemicals."
"Describe the position of equilibrium."	"The position of equilibrium describes the composition of the equilibrium mixture. If it favors the reactants, the equilibrium mixture will contain mostly reactants."
"What is Le Chatelier's principle?"	"Le Chatelier's principle states that if an external condition is changed, the equilibrium will shift to oppose the change."
"How does temperature affect equilibrium?"	"If temperature is increased, the equilibrium will shift in the endothermic direction to try to reduce the temperature. If temperature is decreased, the equilibrium will shift in the exothermic direction to try to increase the temperature."
"What is the effect of pressure on equilibrium?"	"Increasing pressure will cause the equilibrium to shift towards the side with fewer moles of gas to oppose the change and reduce the pressure. Decreasing pressure will cause the equilibrium to shift towards the side with more moles of gas to oppose the change and increase the pressure."
"Describe the effect of increasing the concentration of OH- ions on equilibrium."	"Increasing the concentration of OH- ions causes the equilibrium to shift to oppose this and move in the forward direction to remove and decrease the concentration of OH- ions. The position of equilibrium will shift towards the right, giving a higher yield of I- and IO3-. The color would change from brown to colorless."
"What is the effect of adding H+ ions on equilibrium?"	"Adding H+ ions reacts with the OH- ions and reduces their concentration, so the equilibrium shifts back to the left, giving a brown color."
"How does a catalyst affect the position of equilibrium?"	"A catalyst has no effect on the position of equilibrium, but it will speed up the rate at which the equilibrium is achieved."
"Why is equilibrium important in industrial processes?"	"Equilibrium is important in industrial processes because it allows for the production of desired products with good yield and rate. It also helps in finding a compromise between temperature and pressure to optimize energy costs."
"Describe the contact process for the production of sulfuric acid."	"The contact process involves the oxidation of sulfur dioxide to sulfur trioxide using oxygen in the presence of a catalyst, typically vanadium pentoxide. The sulfur trioxide is then reacted with water to produce sulfuric acid."
"What is dynamic equilibrium?"	"Dynamic equilibrium is a state in which both forward and backward reactions occur at equal rates."
"What is the purpose of using a catalyst in industrial processes?"	"The purpose of using a catalyst in industrial processes is to speed up the rate of the reaction without affecting the position of equilibrium. This allows for faster production and lower energy costs."
"Describe the hydration of ethene to produce ethanol."	"The hydration of ethene involves the addition of water to ethene in the presence of a catalyst, typically phosphoric acid. This reaction produces ethanol, an important alcohol used in various industries."
"How is methanol produced from carbon monoxide and hydrogen?"	"Methanol is produced from carbon monoxide and hydrogen gases in the presence of a catalyst, typically chromium and zinc oxides. This reaction occurs at high temperature and pressure and produces methanol, which is used as a fuel and solvent."
"What is the effect of high pressure in the production of ethene to poly(ethene)?"	"High pressure in the production of ethene can lead to unwanted polymerization of ethene to poly(ethene), which is not desired in the process."
"Describe equilibrium equations."	"Equilibrium equations are mathematical expressions that represent the balance between the rates of the forward and reverse reactions in a chemical system at equilibrium."
"Define equilibrium constant Kc."	"The equilibrium constant Kc is a numerical value that represents the ratio of the concentrations of the products to the concentrations of the reactants at equilibrium."
"How do you calculate the unit of K for a chemical equation?"	"To calculate the unit of K for a chemical equation, you put the unit of concentration (mol dm-3) into the K equation and cancel out the units to determine the final unit."
"Describe how to calculate the moles of reactant at equilibrium."	"To calculate the moles of reactant at equilibrium, subtract the moles reacted from the initial moles of the reactant."

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