Tro - Chapter 14

Tro - Chapter 14 - 14.1 How do the rates of the forward and...

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14.1 How do the rates of the forward and reverse reactions compare when a system is in equilibrium? 14.2 If no concentrations are changing, why is equilibrium considered to be a dynamic process? 14.3 What is the difference between K and k? 14.4 In mass action expressions, what symbolism is often used to indicate molarity? 14.5 Where do the coefficients from a balanced chemical equation appear in a mass action expression? 14.6 (a) How does the equilibrium constant change when the equation is reversed? (b) How does the equilibrium constant change when the coefficients in a reaction are doubled? 14.7 Write the equilibrium constant expressions (Kc) for each of the following reactions: (a) CaCO 3 (s) CaO (s) + CO 2 (g) (b) C (s) + CO 2 (g) 2 CO (g) (c) PCl 5 (s) + H 2 O (l) 2 HCl (g) + POCl 3 (g) (d) 2 NaHCO 3 (s) Na 2 CO 3 (s) + CO 2 (g) + H 2 O (l) (e) Nitrogen plus Hydrogen in equilibrium with Ammonia
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14.8 Write mass action expressions for each of the following: (a) 2 O 3 (g) 3 O 2 (g) (b) CaCO 3 (s) CaO (s) + CO2 (g) (c) Sulfur dioxide gas plus oxygen gas in equilibrium with sulfur trioxide gas. (d) Pb 3 (PO 4 ) 2 (s) 3 Pb 2 + (aq) + 2 PO 4 3- (aq) (e) MnC 2 O 4 (s) + C 2 O 4 2- (aq) [Mn (C 2 O 4 ) 2 ] 2- (aq) 14.10 The following equilibrium was studied at 973 K: 2 SO 3 (g) 2 SO 2 (g) + O 2 (g) at this temperature the value of Kc is 2.4 x 10 -3 . (a) What is the value of Kc for the following reaction at 973 K? 4 SO 3 (g) 4 SO 2 (g) + 2 O 2 (g) (b) What is the value of Kc for the following reaction at 973 K? 2 SO 2 (g) + O 2 (g) 2 SO 3 (g) . (c) What is the value of Kc for the following reaction at 973 K? SO 2 (g) + 1/2 O 2 (g) SO 3 (g) . 14.11 Write the equation for relating Kp to Kc. Define each term in this equation.
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14.12 Write mass action expressions, Kc and Kp, for each of the following equilibriums. Determine which of these equilibriums are homogeneous and which are heterogeneous. (a) 2 NO 2 (g) N 2 (g) + 2 O 2 (g) (b) H 2 SO 3 (aq) H + (aq) + HSO 3 - (aq) (c) C (s) + H 2 O (g) CO (g) + H 2 (g) (d) Fe 3+ (aq) + 3 C 2 O 4 2- (aq) Fe (C 2 O 4 ) 3 3- (aq) (e) 2 Zn (s) + O 2 (g) 2 ZnO (s) (f) Mg 3 (AsO 4 ) 2 (s) 3 Mg 2+ (aq) + 2 AsO 4 3- (aq) (g) 2 C 4 H 10 (g) + 13 O 2 (g) 8 CO 2 (g) + 10 H 2 O (l) (h) MnCO 3 (s) CO 2 (g) + Mn (s) 14.13 A sample of NO2 having a partial pressure of 0.750 atm at 1000. K was sealed in a container and the following equilibrium was established. At equilibrium, the total pressure in the system was 1.098 atm. Calculate Kp. 2 NO 2 (g) 2 NO (g) + O 2 (g)
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14.14 Determine ∆ng for each of the following equilibrium. (a) H
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Tro - Chapter 14 - 14.1 How do the rates of the forward and...

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