Given the reactions 2D(6) A() Kc1 = 51.3 and B(g) +D(E)=E Kc2 = 1.23 x 10...
1) Given the two reactions: a) H2S<--> HS- + H+, K1=9.13 x 10-8 b) HS-<--> S2- + H+, K2=1.20 x 10-19 what is the equilibrium constant Kfinal for thefollowing reaction? S2- + 2H+<--> H2S 2) Given the two reactions: a)PbCl2 <--> Pb2+ + 2Cl-,K1= 1.80 x 10-10 b) AgCl<--> Ag+ + Cl-, K2= 1.23 x10-4 what is the equilibrium constant Kfinal for thefollowing reaction? PbCl2 + 2Ag+<--> 2AgCl + Pb2+
At a given temperature the equilibrium constant is given for two of the reactions below. a. Write the equilibrium expression (equation) for Kc3 b. Determine the value of Kc3. Show work to support your answer. HX(aq) + H2O(l) ⇌ X-(aq) + H3O+ (aq) Kc1 = 1.21x10-7 X-(aq) + + H2O(l) ⇌ OH-(aq) + HX(aq) Kc2 = 1.21x10-7 HX(aq) + H2O(l) ⇌ OH-(aq) + H3O+ (aq) Kc3 = __________________
Consider the 2 following reactions: A +B --> C+2D (Δ G r x n= 525 k J) 2B -->3D (Δ G r x n = 490 k J) What is the Equilibrium constant of the reaction A+D --> C+B at T=298K? Instruction: Write your answer in units of 10-7
Calculate the value of the equilibrium constant, K, for the reaction Q(g) + X(g) = 2 M(g) + N(g) given that M(g) = 2(g) 6 R(g) = 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kel = 3.00 Kc2 = 0.512 K3 = 11.1 Kc = 53.207
Part A= Given the two reactions H2S⇌HS−+H+, K1 = 9.42×10−8, and HS−⇌S2−+H+, K2 = 1.32×10−19, what is the equilibrium constant K final for the following reaction? S2−+2H+⇌H2S Part B= Given the two reactions PbCl2⇌Pb2++2Cl−, K3 = 1.89×10−10, and AgCl⇌Ag++Cl−, K4 = 1.23×10−4, what is the equilibrium constant K final for the following reaction? PbCl2+2Ag+⇌2AgCl+Pb2+
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...
For this heterogeneous system 2 A(aq) + 3 B(g) + C(1) = 2D(s) + 3 E(g) the concentrations and pressures at equilibrium are [A] = 6.74 x 10-2 M, PB = 8.08 x 10° Pa, [C] = 11.97 M, D = 18.57 M, and PE = 1.79 x 104 torr. Calculate the thermodynamic equilibrium constant, K. K =
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)
the equilibrium constant is given for two of the reactions below. Determine the value of the missing 23) - equilibrium constant A(g) +B(g) - AB(g) AB(g) + A(g) - A2B(g) 2 A(g) +B(g) - A2B(g) Ke=0.24 Ke = 3.8 Ke=? A) 0.63 B) 4.0 C) 16 D) 0.91 E) 3.6 24) 24) Determine the value of Kp for the following reaction, at 300K, if the equilibrium concentrations are as follows: (N2leq -1.5M, [H2leq = 1.1 M, (NH3 leq = 0.47...
For the reaction 3A(g) + 2B(g) → 2C(g) + 2D(g) the following data was collected at constant temperature. Determine the correct rate law for this reaction and value of rate constant. Trial Initial [A] Initial [B] Initial Rate (mol/L) (mol/L) (mol/(L• min)) 1 0.200 0.200 1.20 × 10–1 2 0.200 0.100 6.00 × 10–2 3 0.100 0.200 3.00 × 10–2 Predict the rate of reaction for Trial #4 using the correct rate law and rate constant. 4 0.300 0.200 ?????????