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21 Cards in this Set
- Front
- Back
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Reaction Rate
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how fast or slow a reaction takes place
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Temperature & Reaction Rates
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conducting a reaction at a higher temperature delivers more energy into the system and increases the reaction rate by causing more collisions between particles, as explained by collision theory
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Surface Area & Reaction Rates
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the rate of reaction increases as the surface area does. That is because more particles of the solid are exposed and can be hit by reactant molecules
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Concentration & Reaction Rate
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Reaction rate increases with concentration, as described by the rate law and explained by collision theory. As reactant concentration increases, the frequency of collision increases
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Collision Theory
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the idea that the more collisions there are between reactants, the more likely they are to react and therefore more reactions take place
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Reversible Reactions
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a chemical reaction that results in an equilibrium mixture of reactants and products where reactions can travel right to left and left to right simultaneously
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Dynamic Equilibrium
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exists when a reversible reaction ceases to change its ratio of reactants/products, but substances move between the chemicals at an equal rate, meaning there is no net change
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Rates of Forward and Reverse Reactions
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when the forward reaction proceeds at the same rate as the reverse reaction. The reaction rates of the forward and reverse reactions are generally not zero but, being equal, there are no net changes in the concentrations of the reactant and product
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Chemical Equilibrium
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the state in which the concentrations of the reactants and products have no net change with time
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Equilibrium Position
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changed if you change the concentration of something present in the mixture. According to Le Chatelier's Principle, the position of equilibrium moves in such a way as to tend to undo the change that you have made
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Le Chatelier's Principle
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If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established
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Effect of Concentration on Equilibrium Position
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According to Le Chatelier's Principle, the position of equilibrium moves in such a way as to tend to undo the change that you have made
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Effect of Temperature on Equilibrium Position
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If you increase the temperature, the position of equilibrium will move in such a way as to reduce the temperature again. It will do that by favouring the reaction which absorbs heat.
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Effect of Pressure on Equilibrium Position
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if you increase the pressure, the position of equilibrium will move in such a way as to decrease the pressure again - if that is possible. It can do this by favouring the reaction which produces the fewer molecules. If there are the same number of molecules on each side of the equation, then a change of pressure makes no difference to the position of equilibrium.
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Activation Energy
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the minimum energy required to start a chemical reaction
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Catalysis
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the change in rate of a chemical reaction due to the participation of a substance called a catalyst
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Enzymes
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proteins that catalyze (i.e., increase the rates of) chemical reactions.[1][2] In enzymatic reactions, the molecules at the beginning of the process are called substrates, and they are converted into different molecules, called the products
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Equilibrium Constant (Keq)
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aA + bB <--> cC + dD
Keq = ( ( [C]^c) x ( [D]^d) ) / ( ( [A]^a) x ( [B]^b) ) |
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Keq = 1
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Neither side is favored
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Keq > 1
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Products are favored
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Keq < 1
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Reactants are favored
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