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K and Q explain the directioninwhich the reaction will proceed ineach case. 3) SO2(g)+O2(g) SO3(g) for...
166666.6 .0012 3. SO2(g)+ O2(g) = SO:(g) for which K -2.5x102 Initially Pso2=1.5atm, Poz-1.2atm, Pso3=1.2atm 6 6666666667 > 2.500 .2 1.2 1.5 1.2 4. N2(g) + 3H2(g) + 2NH3(g) for which K=2.3 Initially [N2]=0.071 M, [H.]=9.17x10 M, (NH3)-1.83x10-M 203
Module 9 Homework K and Q. Explain the direction in which the reaction will pro 1. CH.COOH(aq) + H20 (1) = CH.COO (aq) + Initially: [CH.COOH]-0.16 M. [CH,COO)-0.0028 the reason will proceed in each case. CHCOO (aq) + H2O (aq) for which K. - 4.2x10 M, CH.COO)-0.0028 M, [H,O)-0.0048 M 2. CO(g)+2H:(g) = CH,OH(g) for which K, -0.0012 Initially: Pco-0.03atm, P=0.004atm, ProR0.08atm. 3. SO2(g)+ O2(g) + SO.(g) for which K -2.5x102 Initially Pso2=1.5atm, Poz-1.2atm, Pso3=1.2atm 4. N2(g) + 3H2(g) +...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. 2NH3(g)⇌N2(g)+3H2(g)Kc=17; [NH3] = 0.20 M, [N2] = 1.00 M, [H2] = 1.00 M (b) 2NH3(g)⇌N2(g)+3H2(g)KP=6.8×104; NH3 = 3.0 atm, N2 = 2.0 atm, H2 = 1.0 atm (c) 2SO3(g)⇌2SO2(g)+O2(g)Kc=0.230; [SO3] = 0.00 M, [SO2] = 1.00 M, [O2] = 1.00 M (d) 2SO3(g)⇌2SO2(g)+O2(g)KP=16.5; SO3 = 1.00...
A reaction vessel contains an equilibrium mixture of SO2, O2,, and SO3. The reaction proceeds such that: 2SO2 (g) + O2 (g) ----> <---- 2SO3 (g) The partial pressures at equilibrium are Pso2=0.001111 atm PO2 = 0.002728 atm PSO3 =0.0166 Calculate the Kp for the reaction.
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.
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 =
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.
For the reaction 2 SO3 (g) equilibrium reaction arrow 2 SO2 (g) + O2 (g) Kp = 0.335 at 1000 K. Calculate Kc at 1000 K. Please help.
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
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.