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kinetics y equilibrm
| Question | Answer |
|---|---|
| What is kinetics? | The study of how fast a chemical reaction occurs |
| What is reaction rate? | The rate of change in reactant and product concentrations |
| What is a reactant? | A substance present at the start of a reaction |
| What is a product? | A substance produced in a chemical reaction |
| What does collision theory state? | Reactions occur when particles collide with sufficient energy and proper orientation |
| What two conditions are required for a successful collision? | Sufficient energy and proper orientation |
| How does increasing temperature affect reaction rate? | It increases the reaction rate |
| Why does increasing temperature increase reaction rate? | Particles collide more frequently and with greater energy |
| How does increasing concentration affect reaction rate? | It increases the reaction rate |
| Why does increasing concentration increase reaction rate? | More particle collisions occur |
| How does increasing surface area affect reaction rate? | It increases the reaction rate |
| Why does increasing surface area increase reaction rate? | More collisions occur per unit time |
| How does increasing pressure affect the rate of a gas reaction? | It increases the reaction rate |
| Why does increasing pressure increase reaction rate? | Gas particles are closer together and collide more often |
| What is a catalyst? | A substance that increases reaction rate without being consumed |
| How does a catalyst increase reaction rate? | It provides an alternate pathway with lower activation energy |
| Is a catalyst consumed during a reaction? | No |
| What does a catalyst do to activation energy? | Lowers it |
| What type of substances generally react fastest? | Aqueous ions |
| What state symbol usually indicates the fastest reacting substances? | (aq) |
| Do gases generally react faster than solids? | Yes |
| Do ionic compounds generally react faster than covalent compounds? | Yes |
| What does a potential energy diagram show? | The energy changes during a reaction |
| What is heat of reaction? | The net energy gained or lost during a reaction |
| What is another name for heat of reaction? | Change in enthalpy |
| What symbol represents heat of reaction? | ΔH |
| What is the formula for heat of reaction? | ΔH = PEproducts - PEreactants |
| What is the sign of ΔH for an endothermic reaction? | Positive |
| What is the sign of ΔH for an exothermic reaction? | Negative |
| In an endothermic reaction, which has greater potential energy: reactants or products? | Products |
| In an exothermic reaction, which has greater potential energy: reactants or products? | Reactants |
| Does the forward reaction have the opposite ΔH of the reverse reaction? | Yes |
| If the forward reaction is endothermic, what is the reverse reaction? | Exothermic |
| If the forward reaction is exothermic, what is the reverse reaction? | Endothermic |
| What is activation energy? | The minimum energy required for a reaction to occur |
| How does a catalyst affect the PE diagram? | It lowers the activation energy peak |
| Does a catalyst change ΔH? | No |
| Does a catalyst change the PE of reactants or products? | No |
| What is entropy? | A measure of randomness or disorder |
| Which phase has the lowest entropy? | Solid |
| Which phase has the highest entropy? | Gas |
| How does entropy change from solid to liquid to gas? | It increases |
| Which has greater entropy: NaCl(s) or NaCl(aq)? | NaCl(aq) |
| What happens to entropy when a soluble solid dissolves? | Entropy increases |
| What conditions favor spontaneity? | Lower energy and higher entropy |
| What type of reaction is more likely to be spontaneous? | Exothermic with increasing entropy |
| What is Gibbs free energy? | A quantity used to predict spontaneity |
| What is the Gibbs free energy equation? | ΔG = ΔH - TΔS |
| When is a reaction spontaneous? | When ΔG is negative |
| If ΔH is negative and ΔS is positive, is the reaction spontaneous? | Always spontaneous |
| If ΔH is positive and ΔS is negative, is the reaction spontaneous? | Never spontaneous |
| What is equilibrium? | A state where forward and reverse reaction rates are equal |
| At equilibrium, are the forward and reverse rates equal? | Yes |
| At equilibrium, do concentrations remain constant? | Yes |
| At equilibrium, must reactant and product concentrations be equal? | No |
| What happens to reactant concentration at equilibrium? | It remains constant |
| What happens to product concentration at equilibrium? | It remains constant |
| When is a solution at equilibrium? | When it is saturated |
| What occurs at equal rates in a saturated solution? | Dissolving and recrystallization |
| What occurs at equal rates during liquid-vapor equilibrium? | Evaporation and condensation |
| What occurs at equal rates at the melting point? | Melting and freezing |
| What does Le Chatelier's Principle state? | A system shifts to oppose a stress applied to it |
| What stresses affect equilibrium? | Concentration, pressure, volume, and temperature |
| What happens when a reactant is added? | Equilibrium shifts away from the reactant side |
| What happens when a product is added? | Equilibrium shifts away from the product side |
| What happens when a reactant is removed? | Equilibrium shifts toward the reactant side |
| What happens when a product is removed? | Equilibrium shifts toward the product side |
| What happens when pressure increases in a gas equilibrium? | Shifts toward fewer moles of gas |
| What happens when volume decreases in a gas equilibrium? | Shifts toward fewer moles of gas |
| What happens when pressure decreases in a gas equilibrium? | Shifts toward more moles of gas |
| What happens when volume increases in a gas equilibrium? | Shifts toward more moles of gas |
| Which side is favored when temperature increases? | The endothermic side |
| Which side is favored when temperature decreases? | The exothermic side |
| Does adding a catalyst shift equilibrium? | No |
| How does a catalyst affect equilibrium? | It speeds up both forward and reverse reactions equally |
| What is the common ion effect? | Solubility decreases when a common ion is added |
| What happens when a common ion is added to a saturated solution? | Equilibrium shifts toward the solid |
| What happens to solubility when a common ion is added? | It decreases |
| In AgCl(s) ⇌ Ag+(aq) + Cl-(aq), what happens when Cl- is added? | The equilibrium shifts left |
| In AgCl(s) ⇌ Ag+(aq) + Cl-(aq), what happens to Ag+ concentration when Cl- is added? | It decreases |
| In AgCl(s) ⇌ Ag+(aq) + Cl-(aq), what happens to the amount of AgCl(s) when Cl- is added? | It increases |
| What Regents keyword indicates equilibrium? | Equal rates |
| What Regents keyword indicates spontaneity? | Negative ΔG |
| What Regents keyword indicates entropy? | Randomness |
| What Regents keyword indicates a catalyst? | Lower activation energy |
| What Regents keyword indicates an exothermic reaction? | Negative ΔH |
| What Regents keyword indicates an endothermic reaction? | Positive ΔH |
Created by:
markoii