Lecture 61/30/06 Seminar TODAY at 4. Effect of a catalyst Increases the rate at which reaction gets to equilibrium  Doesn’t change the equilibrium concentrations.

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Lecture 61/30/06 Seminar TODAY at 4

Effect of a catalyst Increases the rate at which reaction gets to equilibrium  Doesn’t change the equilibrium concentrations  How does it affect K? Many industrial processes use heterogeneous catalysts

Example For the following reaction: ΔH˚ = 2816 KJ/mol 6 CO 2 (g) + 6 H 2 O (l) ⇄ C 6 H 12 O 6 (s) + 6 O 2 (g) How is the equilibrium yield of C 6 H 12 O 6 affected by: Increasing P CO2 ? Increasing temperature? Removing CO 2 ? Decreasing the total pressure? Removing part of the C 6 H 12 O 6 ? Adding a catalyst?

C (s) + CO 2 (g) ⇄ 2 CO (g) P total = 1 atm Endothermic or exothermic? Calculate K p and K c at 850 ˚C T (˚C)CO 2 (mol %)CO (mol %)

Problem A sample of pure SO 3, weighing g was placed in a 1.00-L flask and heated to 1100 K to decompose it partially. 2SO 3 (g) ⇄ 2 SO 2 (g) + O 2 (g) If a total pressure of atm was developed, find the value of K c for this reaction at this temperature.

Precipitation reactions What are they? Solubility?

Solubility Rules Soluble CompoundsExceptions NO 3 - None C 2 H 3 O 2 - (acetate)None Cl -, Br -, I - Compounds with Ag +, Hg 2 2+, Pb 2+ SO 4 2- Compounds with Sr 2+, Ba 2+, Hg 2 2+, Pb 2+ Group 1A and NH 4 + None Insoluble CompoundsExceptions S 2- Group 1A and NH 4 +, Ca 2+, Sr 2+, Ba 2+ CO 3 2-,PO 4 3-, C 2 O 4 2-, CrO 4 2- Group 1A and NH 4 + OH - Group 1A and NH 4 +, Ca 2+, Sr 2+, Ba 2+

Equations Pb(NO 3 ) 2 reacts with NaI (aq) to form the insoluble compound, PbI 2. Molecular Equation? Complete Ionic Equation? Net Ionic Equation?

Solubility vs. Solubility constant (K sp ) What is the difference? BaSO 4 (s) ⇄ Ba 2+ (aq) + SO 4 2- (aq) Ba 2+ (aq) + SO 4 2- (aq) ⇄ BaSO 4 (s)

What is the K sp for AgI if the solubility equals 9.2 x M at 25˚ C?

The K sp of AgBr at 100 ˚C is 5 x Calculate the solubility of AgBr at that temperature in molarity.

A saturated solution of silver oxalate (Ag 2 C 2 O 4 ) contains 6.9 x M of C 2 O 4 2- at 25˚C. Calculate the K sp of silver oxalate at that temperature.

The K sp of MgF 2 = 5.2 x Calculate the solubility in molarity and grams per liter.

Comparison of solubility based on K sp AgI (K sp = 8.5 x ) < AgBr (K sp = 5.4 x ) < AgCl (K sp = 1.8 x ) PbI 2 (K sp = 9.8 x ) < PbBr 2 (K sp = 6.6 x ) < PbCl 2 (K sp = 1.7 x ) Can only compare salts with same ion ratio AgCl (K sp = 1.8 x ) vs. Ag 2 CO 3 (K sp = 8.5 x ) Solubility of AgCl = 1.3 x mol/L Solubility of Ag 2 CO 3 = 1.3 x mol/L