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=?
Given the equilibrium constants for reactions 1 and 2, determine the equilibrium constant for reaction 3....
At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g)+O2(g)<==>2SO3(g) is 2.99x10^-3. What is the value of the equilibrium constant for each of the following reactions at that temperature? a. SO2(g)+ 1/2 O2(g)<==> SO3(g) b. 2SO3(g)<==>2SO2(g)+O2(g) c. SO3(g)<==> SO2(g)+ 1/2 O2(g)
If the equilibrium constant for reaction X is K. What is the equilibrium constant for reaction Y is? Reaction X: SO2 (g) + (1/2) O2 (g) ⇌ SO3 (g) Reaction Y: 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) a. 2K b. K2 c. 1/K2 d. 0.5 x K e. -K2
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
(10) 5. Use the given reactions and their enthalpies to determine the AHºrxn for the following reaction: 2 S(x) + 3 O2(g) → 2503(g) Hºrxn - ? Given Reactions and their Standard Enthalpies of Reaction: SO2(g) - S(s) + O2(g) 2 SO2(g) + O2(g) 2 S03(g) AHºrxn = +296.8 kJ Hºrxn = -197.8 kJ (10) 6. Use standard enthalpies of formation (AH°f) to determine AHºrxn for the reaction below. 2 CH3OH(1) + 3 02(g) → 2 CO2(g) + 4H2O(g)
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; =
Given the equilibrium constants for the following reactions: 2H2(g) + O2(g) → 2H2O(g) K1 = 3.74 x 1026 H2(g) + Cl2(g) → 2HCl(g) K2 = 9.73 x 1012 calculate the equilibrium constant for the reaction below. 4HCl(g) + O2(g) → 2Cl2(g) + 2H2O(g)
Given these equilibrium reactions: 1. % Sa(s) + 2O2te) <---------- → 2 SO2 Ka = 1.86 x 10105 2. 1/8 Ses) + 3/2 O2(e) <--------→ SO3(e) ka = 1.77 x 1053 Calculate the equilibrium constant ka for the reaction below, which is important in the formation of acid-rain air pollution. 2 SO2(g) + O2(g) ------ --→2 SO3(g) [SO] Klz- 30g] 7 [0]
At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g) <----> 2CO(g) +O2(g) are 1.6*10^-11 and 1.3*10^-10, respectively. a. what is the value of the equilibrium constant for the reaction: (3) CO2(g) + H2(g) <----> H2O(g) + CO(g) at this temperature? b. demonstrate how the calculations of equilibrium constants matches the calculations of dG0r when adding two reactions or more ; determine dG0r for reactions (1) and (2) and use these values in order...
Use the equilibrium constants for the following reactions at 700 °C 2SO2(g) + O2(g) 2SO3(g) K1 = 4.8 2NO(g) + O2(g) 2NO2(g) K2 = 16 to determine the equilibrium constant for the following reaction. SO 3( g) + NO( g) SO 2( g) + NO 2( g)
[Refer Given the following equilibrium constants at 425°C, 1 Na2O(s) – 2 Na(1) +02(9) K= 5 x 10-25 NaO(9) = Na(1)+ - 02(9) K2 = 2 x 10-5 Na, O2(8) = 2 Na(l) + O2(9) K3 = 8 x 10-29 NaO2(s) = Na(l) + O2(9) K4 =1 10-14 determine the values for the equilibrium constants for the following reactions: a. Na2O(s) + + 02 (9) = Naz02 (8) Equilibrium constant = b. NaO(g) + Na2O(8) = Na2O2(8) + Na(1) Equilibrium...