[Refer Given the following equilibrium constants at 425°C, 1 Na2O(s) – 2 Na(1) +02(9) K= 5...
8b. Given that Na(l) + 12 O2 (g) = Nao (g) K1 = 2 x 105 Na2O2(s) + Na(l) = NaO(g) + Na2O(s) K2 = 2 x 10-8 2Na(l) + 1/2O2 (g) = Na2O(s) K3 = 2 x 1025 Determine the value for the equilibrium constant for the following reaction Na2O2(s) = 2NaO(g)
Part 1: Which of the following gas samples would be most likely to behave ideally under the stated conditions? Explain. A) N2 at 1 atm and -70°C B) CO at 200 atm and 25°C C) SO2 at 2 atm and 50 °C D) Ne at STP E) NH3 at 1 atm and 25°C PART 2: Given that Na(l) + ½ O2 (g) ⇌ NaO (g) K1 = 2 x 105 Na2O2(s) + Na(l) ⇌ NaO(g) + Na2O(s) K2 =...
9. At a particular temperature, the following reactions have the equilibrium constants shown: S(s) + O2(g) = SO2(g) K-4.2 1052 2 S(s) + 3 02(g) = 2 SO3(g) K2 = 9.8* 10128 Calculate the equilibrium constant K; for the following reaction at the same temperature. 2 SO2(g) + O2(g) = 2 SO3(g) K; =
9. The equilibrium constants for the following reactions are K, and K2 as shown, 2NO (g) +02 (g)2NO2 (2) Ki 2S02 (g) + 02 (g)2SO3 (g) K2 the equilibrium constant for the reaction, NO2 (g)+ SO2 (g)sNO (g)+SO3 (g), is K2 c. a. K,K2 e. none of these 2 2K 14 10. The solubility product expression (Kip) for the dissolution of Group I salt KCI) in water is K+ ICI 11. A 7 L sample of a gas is confined...
Determine the value of the equilibrium constant,Kgoal , for the reaction CO2(g)--->/<--- C(s)+O2(g), Kgoal=? by making use of the following information: 1. 2CO2(g)+2H2O(l)--->/<--- CH3COOH(l)+2O2(g), K1=5.40x10^-16 2. 2H2(g)+O2(g)--->/<--- 2H2O(l), K2=1.06x10^10 3. CH3COOH(l)--->/<--- 2C(s)+2H2(g)+O2(g), K3= 2.68x10^-9 Kgoal=_______
Part A Determine the value of the equilibrium constant, Kgoal, for the reaction CO2(g)⇌C(s)+O2(g), Kgoal=? by making use of the following information: 1. 2CO2(g)+2H2O(l)⇌CH3COOH(l)+2O2(g), K1 = 5.40×10−16 2. 2H2(g)+O2(g)⇌2H2O(l), K2 = 1.06×1010 3. CH3COOH(l)⇌2C(s)+2H2(g)+O2(g), K3 = 2.68×10−9 Express your answer numerically. Part B Determine the equilibrium constant, Kgoal, for the reaction 4PCl5(g)⇌P4(s)+10Cl2(g), Kgoal=? by making use of the following information: P4(s)+6Cl2(g)⇌4PCl3(g), K1=2.00×1019 PCl5(g)⇌PCl3(g)+Cl2(g), K2=1.13×10−2 Express your answer numerically.
It is possible to predict the equilibrium constant of a reaction by combining two or more reactions for which the value of K is known. When combining equilibrium constants, it is important to note the following: When a reaction is reversed, its Kvalue is inverted; that is, Kreverse=1/Kforward. When the coefficients of a reaction are multiplied by a factor, the K value is raised to the power of that factor. When reactions are added, their Kvalues are multiplied. Part A...
Given the equilibrium constants for reactions 1 and 2, determine the equilibrium constant for reaction 3. (1) 2H2S (g) + SO2(g) = 3S(s) + 2H2O(g) K=1.00 X 10^5 (2) 3SO2(g) + O2(g) = 2SO3(g) K=11.0 (3) 4H2S(g) + 2SO3(g) = 6S(g) + 4H2O(g) + O2 K=?
9. (1.2 pt) At a certain temperature the following reactions have the Kc constants shown; k, i = 4.2 x 1052 K. ii = 9.8 x 10128 K. = ???? → (i) S(s) + O2(g) SO2 (g) ㄹ (ii) 2 S (s) +3 O2 (g) 2SO3 (g) → Calculate the equilibrium constant Ke for the following reaction at the same temperature. 2502 (g) +02 (g) 2 SO3 (g) Kc
02 INTRO UNIV CHEM Il (LEC D1 Wi18) Te left Use the following equilibrium constants co2(g) + H2(g) <→ CO(g) + H2O(g) K,(400 K) 6.5 x 10 E(s) + 1 /202(g) <==> CO(g) K,(400 K) 1.3 x 1019 CO(g)+ 1/2 O2(g)CO2(g) K,(400 K) 2.8 x 102 CO(g) + 2 H2(g)CH3OH(g) K,(400 k) -2.3 H2(g) + 1 /202(g)-> H2O(g) (400 K)-1.8 x 1029 to determine the equilibrium constant for the following reaction. (You will not need to use all of the...