Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Chapter 13
General Chemistry 2 Spring Semester 2026
| Question | Answer |
|---|---|
| Define a reversible reaction | Processes that proceed in both the forward and reverse direction |
| Define dynamic equilibrium | The condition in which the rate of the forward reaction equals the rate of the reverse reaction |
| What do longer changes in a dynamic equilibrium | The concentrations of reactants and products no longer change |
| Why is the equilibrium dynamic? What is changing? | • Reactants become products • Products become reactants • Both happen at the same rate |
| Qualities of an equilibrium | All chemical reactions will eventually reach equilibrium Equilibrium can be: Almost all reactants, Almost all products, Or somewhere in between Equilibrium describes how much of the products are formed |
| Define Equilibrium Constant | The ratio of the equilibrium concentrations of the products raised to their stoichiometric coefficients divided by the equilibrium concentrations of the reactants raised to their stoichiometric coefficients |
| How is the equilibrium constant expressed | Equilibrium tends to be expressed as a ratio of products to reactants |
| What is K related to equilbirum | K is the equilibrium constant for this reaction K is a constant for a given chemical reaction (at a given temperature)K is different for every chemical reaction |
| What is a heterogeneous equilbiria? | Reaction that includes different phases |
| What is not included in the equilibrium constant expression? | Solids and liquids |
| If Q > K then | Too much products Reactants will form until equilibrium reached Reaction moves to the left |
| If Q < K then | Too much reactants Products will form until equilibrium reached Reaction moves to the right |
| If Q = K then | then equilibrium is reached |
| If K is very large | Almost all products Very little reactants |
| If K is around 1 | Almost equal amounts or products to reactants |
| If K is very small | Almost all reactants Very little products |
| If the equation is manipulated what else is? | K |
| If the equation is doubled what is done to K? | It is squared |
| If the equation is halved what is done to K? | It is raised to the 1/2 |
| If the equation is flipped what is done to K? | It is raised to the negative 1 |
| How can we expresses the equilibrium in a gaseous reaction? | The ratio of the concentrations, or the partial pressures of the gases. |
| Δn equation | Δn = (products) - (reactants) Only for gases |
| What can Le Châtelier's principle be used for? | To predict changes in equilibrium concentrations when a system that is at equilibrium is subjected to a stress. (i.e. a disturbance occurs) |
| What does Le Châtelier's principle say? | When equilibrium is disturbed the reaction will proceed to minimize the disturbance |
| What are some of the disturbances of Le Châtelier's principle? | Adding reactant Adding product Removing reactant Removing product |
| What happens when reactant is removed to a solution according to Le Châtelier's principle? | Moves to the right, turn reactant into product |
| What happens when reactant is added to a solution according to Le Châtelier's principle? | Reaction moves to the left, turning products back to reactants |
| What happens when product is added to a solution according to Le Châtelier's principle? | Reaction moves to the left, turning products to reactants to recover the lost reactant |
| What happens when product is removed to a solution according to Le Châtelier's principle? | Reaction moves to the right, to recover lost product |
| If the reaction is exothermic what will happen if you raise the temperature? | Shifts to the left (less product formation) and more reactant production |
| If the reaction is exothermic what will happen if you lower the temperature? | Shift to the right (more product formation) and less reactant production |
| If the reaction is endothermic what will happen if you raise the temperature? | Shifts to the right (more product formation) and less reactant production |
| If the reaction is endothermic what will happen if you lower the temperature? | Shifts to the left (less product formation) and more reactant formation |
| What happens to K with a shift to the right? | K got larger |
| What happens to K with a shift to the left? | K got smaller |
| What does pressure effect in an equilibrium? | Only affects gas |
| How is pressure manipulated in an equilibrium? | By changing the volume |
| How do you raise the overall pressure? What does the reaction do? | Decrease volume Reaction will try to minimize the number of gas moleulces |
| How do you lower the overall pressure? What does the reaction do? | Lower volume Reaction will try to maximize the number of gas molecules |
| What happens when you add an inert gas to an equilibrium? What does it effect? | Adding an inert gas to raise the pressure of a reaction container does not shift the equilibrium. It does not effect the concentration of gases |
| How do catalysts affect the equilibrium? | Catalysts don’t effect equilibrium |
Created by:
KristenR2025