The equilibrium constant, Kc, for reactions are listed as following:        N2 (g)  + 2O2 (g)    2NO2 (g)    Kc1 = 2.8 × 10-15. N2 (g)  + O2 (g)    2NO(g)      Kc2 = 4.3× 10-25 What will the equilibrium constant for the following reaction be at the same temperature?        2NO(g)  +  O2(g)   2NO2(g)    Kc3 = ?

Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5⁢(g)⁢↽−−⇀⁢PCl3⁢(g)+Cl2⁢(g) A 13.1 gsample of PCl5 is added to a sealed 1.25 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 48.4% of the PCl5 remains. What is the equilibrium constant, Kc , for the reaction?

Nitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no change

You are given the following:   H2 (g) + Br2 (g) 2 HBr (g) Kp = 7.9 x 1011                            H2 (g) 2 H (g) Kp = 4.8 x 10-41                                         Br2 (g) 2 Br (g) Kp = 2.2 x 10-15 What is Kp for the reaction shown below?                                H (g) +  Br (g)   HBr (g) Kp = ?

At 100° C, the Keq for the Haber process is 4,51 x 10-5: N2 + 3 H2        ó           2 NH3 Consider the following reaction conditions and determine if the system is at equilibrium. If not, indicate the direction in which the reaction must proceed to establish equilibrium pNH3 = 105 atm, pN2 = 35 atm and pH2 = 495 atm     pNH3 = 35 atm, pN2 = 0 atm and pH2 = 595 atm   pNH3 = 26 atm, pN2 = 202 atm and pH2 = 42 atm   pNH3 = 105 atm, pN2 = 5 atm and pH2 = 55 atm

Which answer below correctly describes the calculation to find the equilibrium expression for K4? Co(g) + 3H2(g) CS2(g) + 2H2S(g) CH4(g) + H20(g) K1 CH4(g) + 2S2(g) K2 CO(g) + H20(g) CS2(g) + 2H2S(g) + 3CO2(g) = 4CO(g) + 2S2(g) + 2H20(g) CO2(g) + H2(g) K3 K4 Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. K1 x (K2)¬1 x (K3)³ a b K1 x K2 x K3 3(K) x K х Кз d K1 x K2 x (K3)³ Use the following series of reactions to determine the value of the equilibrium constant K.j: NOz + H30+ - C5H5NH+ + OH- 2H20(1) = H30+ + OH° C5H5N + HNO, = C5H5NH+ + NO, Reaction1: HNO2 + H20(1) Kcı =?? -6- Reaction2 : C5 H5N + H20(1) Kc2 = 1.70 × 10 Reaction3 : Ксз — 1.01 X 10 14 Reaction4 : Kc4 = 1.19 x %3D Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 7.07 X 10-4 b 2.01 X 10-25 9.93 X 1024 d 4.17 X 10-24 6.86 X 1034 e

Consider the following equilibrium system at 817 K. SO2 Cl2 (g) 2 SO2(g) + Cl2 (g) If an equilibrium mixture of the three gases at 817 K contains 1.60 x 10-3 M SO2 Cl2, 3.57 x 10-2 SO2, and 2.12 x 10-2 M Cl2, what is the value of the equilibrium constant К? M K =

Consider the reaction: SO₂(g) + 1/2O₂(g) ⇒ SO3 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: 2S(s) + 30₂(g) ⇒ 2SO3 (9) K₁ S(s) + O₂(g) → SO₂(g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K= An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.