Chapter 9 - Equilibria
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| Dynamic Equilibrium: | The Forward and Reverse rates of a reversible chemical reaction are equal in a closed system. The concentrations are unchanging but do not have to be equal.
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| Do the Concentrations of Reactants and the Products change once in Equilibrium? | No, the concentrations of the Products and the Reactants are constant once Equilibrium is reached.
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| What happens to the rate of the forward and reverse reactions when equilibrium is reached? | They are constant and equal.
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| Do the concentrations of the reactants and the Products have to be equal when equilibrium is reached? | No, they can be in different concentrations.
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| In what type of system does Dynamic Equilibrium occur? | In a CLOSED System.
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| Le Chantelier's Principle | If a change if affected on a System in Equilibrium, then the equilibrium will shift in order to counter act the change.
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| Altering the Concentration of a Product/Reactant: | Will cause the equilibrium to shift to the opposite side of that substance. E.g if H2 is increased in H2 + N2 --> NH3 the Ammonia will increase.
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| Altering the Temperature of a System: | Increasing the Temperature will shift the reaction towards the Endothermic reaction. Decreasing the Temperature will shift equilibrium to favor the exothermic reaction.
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| Altering the Pressure of Gases: | The equilibrium will shift in the direction which has the lowest moles, i.e. Increasing pressure in 3H2 + N2 --> 2NH3 shifts the reaction to the right, as the 4 moles on the left hand side are more likely to react.
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| Adding a Catalyst: | Does not affect the Equilibrium, but will increase the rate at which the equilibrium is reached.
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| Write the equation for production of Ethanol: | C2H2 (Ethene) + H2O (Steam) <---> C6H5O (Ethanol). (Delta)H = -46KJmol-1
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| Why does the conditions that Ethanol produced under include a high temperature even though it is an Exothermic Reaction (would benefit from low temp)? | Because running a reaction in low temps cause the rate of reaction, thus the speed at which equilibrium is reached, to be slow as only a few particles will be able to have the required energy to react.
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| Write an equation for the production of Methanol: | CO (Carbon Monoxide) + 2 H2 (Hydrogen) <---> CH3OH (Methanol). (Delta) H = -91KJ Mol-1
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| What is one of the major uses of the alcohols Ethanol and Methanol? | They are used as Motor Fuels.
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| What are compromise Conditions? | These are Conditions that may not produce the highest yield but will produce a product quickly by reaching Dynamic Equilibrium quicker.
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| Define Rate of Reaction: | The Change in concentration of products and reactants over time.
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