Cmc chapter 17

Chapter Menu Chemical Equilibrium Section 17.1 A State of Dynamic Balance Section 17.2 Factors Affecting Chemical Equilibrium Section 17.3 Using Equilibrium Constants Exit Click a hyperlink or folder tab to view the corresponding slides.

Section 17-1 Section 17.1 A State of Dynamic Balance ,[object Object],free energy: the energy that is available to do work—the difference between the change in enthalpy and the product of the entropy change and the absolute temperature ,[object Object],[object Object]

Section 17-1 Section 17.1 A State of Dynamic Balance (cont.) reversible reaction chemical equilibrium law of chemical equilibrium equilibrium constant homogeneous equilibrium heterogeneous equilibrium Chemical equilibrium is described by an equilibrium constant expression that relates the concentrations of reactants and products.

Section 17-1 What is equilibrium? ,[object Object]

Section 17-1 What is equilibrium? (cont.) ,[object Object],[object Object]

Section 17-1 What is equilibrium? (cont.) ,[object Object]

Section 17-1 Equilibrium Expressions ,[object Object],[object Object]

Section 17-1 Equilibrium Expressions (cont.) ,[object Object],[object Object]

Section 17-1 Equilibrium Expressions (cont.) ,[object Object],K eq > 1: Products are favored at equilibrium K eq < 1: Reactants are favored at equilibrium ,[object Object]

Section 17-1 Equilibrium Constants ,[object Object]

[object Object],[object Object],[object Object],[object Object],Section 17-1 Section 17.1 Assessment A reaction is in equilibrium when: A. there are more products than reactants B. the amount of products equals the reactants C. the rate of the forward reaction is greater than the reverse reaction D. the rate of the forward and reverse reactions are equal

[object Object],[object Object],[object Object],[object Object],Section 17-1 Section 17.1 Assessment The value of the equilibrium constant is constant for a given ____. A. temperature B. pressure C. volume D. density

Section 17-2 Section 17.2 Factors Affecting Chemical Equilibrium ,[object Object],reaction rate: the change in concentration of a reactant or product per unit time, generally calculated and expressed in moles per liter per second. Le Châtelier’s principle ,[object Object],When changes are made to a system at equilibrium, the system shifts to a new equilibrium position.

Section 17-2 Le Châtelier’s Principle ,[object Object],[object Object]

Section 17-2 Le Châtelier’s Principle (cont.) ,[object Object],[object Object]

Section 17-2 Le Châtelier’s Principle (cont.) ,[object Object],[object Object],[object Object]

Section 17-2 Le Châtelier’s Principle (cont.) Lowering the piston decreases the volume and increases the pressure. The reaction between CO and H 2 is at equilibrium. As a result, more molecules of the products form. Their formation relieves the stress on the system.

Section 17-2 Le Châtelier’s Principle (cont.) ,[object Object]

[object Object],[object Object],[object Object],[object Object],Section 17-2 Section 17.2 Assessment Which does NOT result in a shift of the equilibrium to the right? A. removing products B. adding reactants C. increasing concentration of reactants D. adding products

[object Object],[object Object],[object Object],[object Object],Section 17-2 Section 17.2 Assessment Any change in ____ results in a change in K eq . A. temperature B. pressure C. volume D. concentration

Section 17-3 Section 17.3 Using Equilibrium Constants ,[object Object],solubility: the maximum amount of solute that will dissolve in a given amount of solvent at a specific temperature and pressure ,[object Object],[object Object]

Section 17-3 Section 17.3 Using Equilibrium Constants (cont.) solubility product constant common ion common ion effect Equilibrium constant expressions can be used to calculate concentrations and solubilities.

Section 17-3 Calculating Equilibrium Concentrations ,[object Object]

Section 17-3 The Solubility Product Constant ,[object Object],[object Object]

Section 17-3 The Solubility Product Constant (cont.) ,[object Object]

Section 17-3 The Solubility Product Constant (cont.)

Section 17-3 The Solubility Product Constant (cont.) ,[object Object],[object Object]

Section 17-3 The Solubility Product Constant (cont.) ,[object Object],[object Object],[object Object]

Section 17-3 The Common Ion Effect ,[object Object],[object Object]

Section 17-3 The Common Ion Effect (cont.) ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 17-3 Section 17.3 Assessment The presence of a common ion ____ the solubility of the dissolved substance. A. decreases B. increases C. does not change D. speeds up

[object Object],[object Object],[object Object],[object Object],Section 17-3 Section 17.3 Assessment If Q sp > K sp A. the solution is unsaturated and no precipitate will form B. the solution is saturated and no precipitate will form C. a precipitate will form, reducing the concentrations of the ions in the solution D. a common ion must be present

Resources Menu Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion

Study Guide 1 Section 17.1 A State of Dynamic Balance Key Concepts ,[object Object],[object Object],[object Object]

Study Guide 2 Section 17.2 Factors Affecting Chemical Equilibrium Key Concepts ,[object Object],[object Object]

Study Guide 3 Section 17.3 Using Equilibrium Constants Key Concepts ,[object Object],[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 1 A change in ____ alters both the equilibrium position and the equilibrium constant. A. pressure B. temperature C. volume D. density

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 2 A(n) ____ equilibrium is when all reactant and products are in the same physical state. A. endothermic B. exothermic C. heterogeneous D. homogeneous

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 3 Which is NOT an example of a homogeneous equilibria? A. H 2 (g) +I 2 (g) ↔ 2HI(g) B. 2H 2 (g) +O 2 (g) ↔ 2H 2 OI(g) C. HCl(aq) + NaOH(aq) ↔ NaCl(aq) + H 2 O D. C 2 H 5 OH(l) ↔ C 2 H 5 OH(g)

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 4 Barium sulfate is toxic to humans, so why can it be ingested for use with gastrointestinal x-rays? A. It is minimally poisonous. B. It has high solubility. C. It has low solubility. D. Your body readily absorbs it.

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 5 The state in which the forward and reverse chemical reactions take place at the same rate is called ____. A. Le Châtelier’s Principle B. Henry’s Law C. Charles’s Law D. chemical equilibrium

[object Object],[object Object],[object Object],[object Object],STP 1 Which does NOT describe a system that has reached chemical equilibrium? A. No new product is formed by the forward reactions. B. The forward and reverse reactions occur at equal rates. C. The concentration of products is equal to the concentration of reactants. D. All the reactants have been used up.

[object Object],[object Object],[object Object],[object Object],STP 2 A(n) ____ equilibrium is when all reactant and products are present in more than one physical state. A. endothermic B. exothermic C. heterogeneous D. homogeneous

[object Object],[object Object],[object Object],[object Object],STP 3 Adding product to a chemical equilibrium: A. does nothing B. creates a stress and shifts the equilibrium to the right C. creates a stress and shifts the equilibrium to the left D. causes more product to form

[object Object],[object Object],[object Object],[object Object],STP 4 Ethylene (C 2 H 4 ) reacts with hydrogen to form ethane (C 2 H 6 ) . C 2 H 4 (g) + H 2 (g) ↔ C 2 H 6 (g) + heat. How could you increase the amount of hydrogen in the system? A. Increase the heat. B. Decrease the heat. C. Increase the C 2 H 4 . D. Decrease the C 2 H 6 .

[object Object],[object Object],[object Object],[object Object],STP 5 Which does NOT result in a shift of the equilibrium to the right? A. removing products B. adding reactants C. increasing concentration of reactants D. decreasing the concentration of reactants

IB Menu Click on an image to enlarge.

CIM Figure 17.14 Equilibrium Shifts Figure 17.19 Precipitation Reaction

Help Click any of the background top tabs to display the respective folder. Within the Chapter Outline, clicking a section tab on the right side of the screen will bring you to the first slide in each respective section. Simple navigation buttons will allow you to progress to the next slide or the previous slide. The “Return” button will allow you to return to the slide that you were viewing when you clicked either the Resources or Help tab. The Chapter Resources Menu will allow you to access chapter specific resources from the Chapter Menu or any Chapter Outline slide. From within any feature, click the Resources tab to return to this slide. To exit the presentation, click the Exit button on the Chapter Menu slide or hit Escape [Esc] on your keyboards while viewing any Chapter Outline slide.

End of Custom Shows This slide is intentionally blank.

Cmc chapter 17

Recommandé

Recommandé

Contenu connexe

Tendances

Tendances (20)

En vedette

En vedette (18)

Similaire à Cmc chapter 17

Similaire à Cmc chapter 17 (20)

Plus de Jane Hamze

Plus de Jane Hamze (15)

Dernier

Dernier (20)

Cmc chapter 17