12. The equilibrium constant for the reaction: SO2(g) + O2(g)so,(g) is Kc # 1.3 x 10,...
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) <----> 2 SO2(g) + O2(g), Kc is 4.08 * 10-3 at 1000 K. Calculate the value for Kp.
At 850 K, the equilibrium constant for the reaction 2 SO, (g) + O2(g) = 250(g) is Kc = 15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium. Left No net reaction Right Answer Bank [S02] = 0.20 M [02] = 0.60 M [SO3) = 0.60 M [SO2] = 0.21 M [02] = 0.10 M [SO3] = 0.60 M [SO2] = 0.80 M [02] = 0.50 M...
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 =
The reaction below has a Kc value of 1.0 � 1012. What is the value of Kp for this reaction at 500 K? 2 SO2(g) + O2(g) 2 SO3(g) Answer 4.1 � 1013 4.2 � 10-11 2.4 � 10-12 2.4 � 1010 1.0 � 1012
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)
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
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.
5 pts Question 3 The reaction and equilibrium constant are provided. 2 SO2 (9) + O2 (g) 92 SO3 (g) Kc = 5.8 x 103 Which direction will the reaction proceed if [SO2] = 0.15 M, [O2] = 0.10 M and (SO3) = 0.50 M? shifts to make more reactant shifts to make more product no shift
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