For the equilibrium 2 SO3(g) <----> 2 SO2(g) + O2(g),
Kc is 4.08 * 10-3 at 1000 K. Calculate the value for Kp.
For the equilibrium 2 SO3(g) <----> 2 SO2(g) + O2(g), Kc is 4.08 * 10-3 at...
For the equilibrium reaction, 2 S03 - 2 SO2 (g) + O2 (g), Kc is 4.08 x10-3 at 1000 K. Calculate the value for Kp. (R 0.0821 L.atm/ mol.K) A. 9.60 B. 2.99 OC. 4.97 x 10-5 OD.0.335
For the equilibrium: 2 SO3(g) < = > O2(g) + 2 SO2(g) Kp = 0.269 at 625 oC What is Kc at this temperature? Kp = Kc[RT]Δn R = 0.08206 L-atm/mol K
2) For the equilibrium: 2 SO3(g) <=> O2(g) + 2 SO2(g) Kp = 0.269 at 625 °C What is Ke at this temperature? Kp = Kc[RT]An R = 0.08206 L-atm/mol K
Given the reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Starting with 0.100 M of SO2 and 0.050 M of O2, which value of K should be used and why? a. KC because the chemicals are in the gas phase. b. KP because the concentrations are in Molarity. c. KP because the chemicals are in the gas phase. d. KC because the concentrations are in Molarity.
12. The equilibrium constant for the reaction: SO2(g) + O2(g)so,(g) is Kc # 1.3 x 10, What is the equilibrium constant for the reaction: 2S0,(g)O,(g)+ 2S02(g) 13. For the following reaction, Kc (@ 500 K) 1.0 x 10 2 SO-(g) + 02(g) 2 SO,(g). What is the value of Kp for this reaction at 500 K? (3 Pts.)
The equilibrium constant for the following reaction is 1.71×10-2 at 847 °C. 2 SO3(g)2 SO2(g) + O2(g) K = 1.71×10-2 at 847 °C Calculate the equilibrium constant for the following reactions at 847 °C. (a) 2 SO2(g) + O2(g)2 SO3(g) K = (b) SO3(g) SO2(g) + 1/2 O2(g) K = Show Approach
. One mole of SO2 gas and 1.00 mol of O2 gas were confined at 1000 K in a 5.00 L flask. The gases reacted, and at equilibrium, 0.840 mol of SO3 gas had formed. Calculate the value of Kc and Kp. 2SO2 (g) + O2 (g) ↔ 2SO3 (g)
14. In which of the following reactions will Kc = Ko? ooo 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H2O(g) 2 SO3(g) + 2 NO(g) = 2 SO2(g) + 2 NO2(g) 4 N2(g) + 2 O2(g) = 4 N2O(g) 6 SO2(g) + 3 O2(g) = 6 SO3(g) None of the above reactions have Kc = Kp.
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to form SO3 is 0.365 at 1.15×103 K: SO2(g) + O2(g) = 2SO3(g) A sample of SO3 is introduced into an evacuated container at 298 K and allowed to dissociate until its partial pressure reaches an equilibrium value of 0.867 atm. Calculate the equilibrium partial pressures of SO2 and O2 in the container. PSO2 = PO2 =
QUESTION 5 3 poi Consider the equilibrium: 2 SO2(g) + O2(g) = 2 SO3(g) A student places 2.00 moles Soz in a 1.00 L flask. When equilibrium is reached (O) = 0.10 M at 130 °C. Calculate the kc. Hint: use the detectivee method and construct an ICE table. Record your answer as a standard number to 2 significant figures. For example, if the answer is 2.75 x 100 M then you should enter 0.00275 as the answer.