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chem test
| Question | Answer |
|---|---|
| Collision Theory (3 parts) | Particles must 1) Collide, 2) have enough Energy, and 3) have the correct Orientation. |
| Activation Energy | The "barrier"—the minimum energy needed for a reaction to actually happen. |
| Concentration & Rate | Higher concentration = more particles = more collisions = Faster Rate. |
| Pressure & Rate (Gases) | Higher pressure = particles squeezed together = more collisions = Faster Rate. |
| Surface Area & Rate | More surface area (crushing a solid) = more exposed particles = Faster Rate. |
| Temperature & Rate | Higher temp = particles move faster AND hit harder = Faster Rate. |
| What does a Catalyst do? | It speeds up a reaction by lowering the Activation Energy. |
| Homogeneous Catalyst | A catalyst that is in the same phase as the reactants (e.g., both are liquids). |
| Heterogeneous Catalyst | A catalyst in a different phase (e.g., a solid metal catalyst with gas reactants). |
| Reversible Reaction | A reaction that can go forwards and backwards at the same time. |
| Dynamic Equilibrium | When the Rates of the forward and reverse reactions are Equal. |
| Equilibrium Concentrations | At equilibrium, the amounts of reactants/products stay Constant (not necessarily equal). |
| Exothermic Graph | The products end lower than the reactants (Energy is released negative). |
| Endothermic Graph | The products end higher than the reactants (Energy is absorbed positive). |
| K equilibrium equation | products over reactants |
| The "Big Rule" for K eq | Solids (s) and Pure Liquids (l) are NEVER included in the expression. |
| K > 1 | The Products are favored (more stuff on the right). |
| K < 1 | The Reactants are favored (more stuff on the left). |
| The only thing that changes K of equilibrium | Temperature. (Concentration and pressure changes do NOT change the K value). |
| Reaction Quotient (Q) | A calculation used to see if a reaction is at equilibrium yet (compared against K). |
| ICE Table acronym | Initial, Change, Equilibrium (used to find missing concentrations). |
| Le Châtelier’s Principle | If you stress a system at equilibrium, it will shift to undo that stress. |
| "Add Away" Rule | If you ADD a substance, the reaction shifts AWAY from that side to use it up. |
| "Take Towards" Rule | If you REMOVE a substance, the reaction shifts TOWARD that side to replace it. |
| Pressure Increase Stress | The reaction shifts toward the side with FEWER moles of gas. |
| Pressure Decrease Stress | The reaction shifts toward the side with MORE moles of gas. |
| Temp Stress (Exothermic) | Heat is a Product. Adding heat shifts it LEFT (away from heat). |
| Temp Stress (Endothermic) | Heat is a Reactant. Adding heat shifts it RIGHT (away from heat). |
| Common Ion Effect | Adding a salt that shares an ion with the solution, causing a shift that forms more precipitate (solid). |
| Q vs. K: Q > K | Too many products! Reaction shifts LEFT (toward reactants). |
| Q vs. K: Q < K | Not enough products! Reaction shifts RIGHT (toward products). |
| Q vs. K: Q = K | The system is already at Equilibrium. |
| Catalyst & Equilibrium | A catalyst makes equilibrium happen faster, but it does NOT cause a shift or change the K value. |
| Which factors must be equal when a reversable chemical process reaches equilibrium | rate of the forward reaction and the rate of the reverse reaction |
| A solute is added to water and a portion of the solute remains undissolved. When equilibrium between the dissolved and undissoived solute is reached, the solution must be | Saturated |
| Which description applies to a system in a sealed flask that is half full of water? | d) Both evaporation and condensation occur. |
| 4) Solution equilibrium always exists in a solution that is | Saturated |
| Given the reaction at equilibrium: A(g) + B(g) <>C(g)+D(g). The addition of a catalyst will | Increase the rate of the forward and reverse reactions equally. |
| If a catalyst is added to a system at equilibrium and the temperature and pressure remain constant, there will be no effect on the | d) Heat of reaction |
| Consider the equation for the following reaction at equilibrium: X + Y-> 2Z + heat. The concentration of the product could by increased by | Increasing the concentration of Y |
| In a reversible reaction, chemical equilibrium is attained when the | Concentration of the products remains constant. |
| Closed System | Equilibrium can only be reached in a Closed System (where no matter can enter or leave). |
| 3 Types of Equilibrium | 1. Phase (Ice<->Water), 2. Solution (Dissolving<->Precipitating), 3. Chemical (Reactants<->Products). |
| What is a "Stressor"? | Any change in Temperature, Pressure, or Concentration that breaks the equilibrium balance. |
| Shift to the Right | Means the reaction works harder to make more Products. |
| Shift to the Left | Means the reaction works harder to make more Reactants. |
| Interpreting Q vs K | If Q < K, the reaction shifts Right. If Q > K, the reaction shifts Left. (Think of alphabetical order: if Q comes before K, move forward/right). |
| Common Ion Effect (Result) | Adding an ion already in the solution decreases solubility, causing more solid (precipitate) to form. |
| how to increase concentration of products | add reactant, remove products and decrease temp if exo |
| how to increase concentration of reactant | Add reactant, remove product, increased temperature if endothermic |
| in a reversible reaction Chemical equilibrium is obtained when the | Concentration of the products remains constant |
| when you see a equation and it adds something to the equation that wasnt in the equation you need to | break it aprat fide what side it goes on and answer the question |
| when you increase the pressure but the # of moles is the same what hapoens to the shift | nothing |
| does increasing the concentraition of something on the reactant side also increase whatver else is on the side | nope |
| The addition of a catalyst to a system at equilibrium will increase the rate of | Both the forward and reverse reactions |
| A system is said to be in a state of dynamic equilibrium when the | Rate at which products are formed is the same as the rate at which reactants are formed |
| If the pressure on gaseous reactants is increased, the rate of reaction is increased because there is an increase in the | concentration |
| whenever a reaction is at equilibrium | The forward and reverse reaction rate are equal |
| In a reversible reaction, chemical equilibrium is attained when the | concentration of the products remains constant |
| when it asks which one will make the reaction occur at the greatest rate which one is it | soultions of ionic compounds |
| The addition of a catalyst to a system at equilibrium will increase the rate of | both the forward and reverse reactions |
Created by:
Fernando.Quezada