1 / 64

640 likes | 831 Vues

JEOPARDY!. Click Once to Begin. Chemistry Final Review Chapter 8: Equilibrium. JEOPARDY!. Equilibrium. Equilibrium Constants. LeChatelier’s Principle and Reaction Quotients. LeChatelier’s Principle and Reaction Quotients, Part II. Calculations with Q and K. Misc. 100. 100. 100. 100.

Télécharger la présentation
## JEOPARDY!

**An Image/Link below is provided (as is) to download presentation**
Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.
Content is provided to you AS IS for your information and personal use only.
Download presentation by click this link.
While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.
During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

**JEOPARDY!**Click Once to Begin Chemistry Final Review Chapter 8: Equilibrium**JEOPARDY!**Equilibrium Equilibrium Constants LeChatelier’s Principle and Reaction Quotients LeChatelier’s Principle and Reaction Quotients, Part II Calculations with Q and K Misc. 100 100 100 100 100 100 200 200 200 200 200 200 300 300 300 300 300 300 400 400 400 400 400 400 500 500 500 500 500 500**What type of reaction occurs when reactants can form**products and products can form reactants? Equilibrium - 100**Equilibrium - 100**Reversible Reactions**Equilibrium - 200**When is chemical equilibrium achieved?**Equilibrium - 200**When the rate of forward reaction equals the rate of reverse reaction.**Equilibrium - 300**At which point is equilibrium achieved?**Equilibrium - 400**Has a system at equilibrium stopped reacting? Why or why not?**Equilibrium - 400**No. The system has reached dynamic equilibrium. The reaction keeps occurring, but the rates of forward and reverse reaction are equal.**Equilibrium - 500**Does a Keq of 1 mean the reactant concentration equals the product concentration?**Equilibrium - 500**No, not necessarily. The powers to which concentrations are raised have a large effect on the value of Keq. Ex. 2 A B; 2 M=[A], 4 M = [B] Keq = 4/(2)2 = 4/4 = 1**What is the general form of an equilibrium constant given:**a A + b B c C + d D? Equilibrium Constants - 100**Keq = [C]cD]d**[A]a[B]b Equilibrium Constants - 100**Which of the following can be included in an equilibrium**expression: Solid Liquid Gas Aqueous solution Equilibrium Constants - 200**Gas and**Aqueous solution Equilibrium Constants - 200**True or false: Equilibrium constants do NOT depend on**temperature. Equilibrium Constants - 300**False. All equilibrium constants are dependent on**temperature Equilibrium Constants - 300**An equilibrium constant much greater than 1 is a _____**favored reaction. Conversely, an equilibrium constant that is much smaller than 1 is _____ favored. Equilibrium Constants - 400**1st blank: Product**2nd blank: Reactant Equilibrium Constants - 400**What are the units of an equilibrium constant?**Equilibrium Constants - 500**There are none!!**Equilibrium Constants - 500**LeChatelier’s Principle & Reaction Quotients - 100**Define LeChatelier’s Principle.**LeChatelier’s Principle & Reaction Quotients - 100**When a system at equilibrium is disturbed, the reaction will counteract that shift in order to re-establish equilibrium.**LeChatelier’s Principle & Reaction Quotients - 200**Which side of the reaction will a system shift towards when reactants are added or products are removed?**LeChatelier’s Principle & Reaction Quotients - 200**To the right. (The products)**LeChatelier’s Principle & Reaction Quotients - 300**What is the difference between the reaction quotient (Q) and equilibrium constant (K)?**LeChatelier’s Principle & Reaction Quotients - 300**Reaction quotients are used at any concentrations while equilibrium constants are only used for equilibrium concentrations.**LeChatelier’s Principle & Reaction Quotients - 400**N2(g) + 3 H2(g) 2 NH3 (g) A system of the above reaction is at equilibrium. Which way will the reaction shift if the volume decreases?**LeChatelier’s Principle & Reaction Quotients - 400**To the right. (The products side)**LeChatelier’s Principle & Reaction Quotients - 500**2 SO2 (g) + O2 (g) 2 SO3 (g) H = -197.8 kJ/mol If heat is added to a system with the above reaction at equilibrium, which direction will the reaction proceed?**LeChatelier’s Principle & Reaction Quotients - 500**To the left. (The reactants side)**LeChatelier’s Principle & Reaction Quotients II - 100**Q = K The system is at ________.**LeChatelier’s Principle & Reaction Quotients II - 100**Equilibrium!!**LeChatelier’s Principle & Reaction Quotients II - 200**Q < K Which direction will the system shift?**LeChatelier’s Principle & Reaction Quotients II - 200**To the right. (The prodcuts side)**LeChatelier’s Principle & Reaction Quotients II - 300**The addition of an inert gas or pure solids to a system at equilibrium results in a shift in which direction?**LeChatelier’s Principle & Reaction Quotients II - 300**No change will occur since neither are included in the equilibrium constant expression.**LeChatelier’s Principle & Reaction Quotients II - 400**When Q > K, the reaction shifts left. Why? Daily Double!!!**LeChatelier’s Principle & Reaction Quotients II - 400**The ratio of products to reactants is too high. Shifting left makes more reactants and increases the value of the denominator in the equilibrium expression, thus lowering the value of Keq**LeChatelier’s Principle & Reaction Quotients II - 500**When will changing the volume of a gas container have no effect on the system?**LeChatelier’s Principle & Reaction Quotients II - 500**When equal number of moles of gas are on each side of the balanced equation.**Calculations with Q and K- 100**Write the equilibrium expression for the given reaction: 2 NOCl (g) 2 NO (g) + Cl(g)**Calculations with Q and K- 100**Keq = [NO]2[Cl] [NOCl]**Calculations with Q and K- 200**Calculate Keq. N2 (g) + O2 (g) 2 NO (g) When [N2] = .48 M; [O2] = .75 M and [NO] = .030 M**Calculations with Q and K- 200**Keq = [NO]2 [N2] [O2] = (.030)2 / (.48) (.75) = .0025**Calculations with Q and K- 300**Calculate Q and determine if the system is at equilibrium or not. COCl2 CO (g) + Cl2(g) & Keq = 170 [CO]=[Cl2]=.15M and [COCl2] = .0011**Calculations with Q and K- 300**Q = [CO][Cl2] [COCl2] =(.15)(.15) / .0011 = 20. The system is not at equilibrium**Calculations with Q and K- 400**Calculate Q and determine which direction the system will shift. H2 (g) + I2(g) 2 HI (g) [H2]= .150 M; [I2]= .175 M; and [HI]= .950 M Keq = 50.5**Calculations with Q and K- 400**Q = [HI]2 [H2][I2] = (.950)2 / (.175)(.150) = 34.4 The system will shift right.

More Related