expression for the equilibrium constant

will the stress causes the equilibrium to shift towards reactants or products, or will it have no effect? 1. PCl5 ⇌ PCl3+Cl2     ΔH>0     (stress:Increase Volume) 2. Co(H2O)2+6(aq) +4Cl-(aq) ⇌ CoCl2-4(aq) +6H20    ΔH>0    (stress:Decrease temperature) 3. N2 + 3H2 ⇌ 2NH3(g)   ΔH<0    (stress: increase pressure by adding helium)

-2 The equilibrium constant K,, for the following reaction is 7.73×10atmat 350°C. What is the value of K. for the reaction at the same temperature? N2(g) +3H2(g)→ 2NH3(g)

Choose the equilibrium constant expressions for the following reactions. a) 2SO2(g) + O2(g)  2SO3(g)      Keq =   b) CS2(g) + 4H2(g)   CH4(g) + 2H2S(g)                            Keq =

Calculate the value of K for the following reaction if the equilibrium concentrations are: [N2] = 0.600 M, [H2] = 0.600 M, and [NH3] = 1.25 M. N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g)

Write the equilibrium constant expression, K , for the following reaction: (If either the numerator or denominator is blank, please enter 1.)   K=

What is the equilibrium expression for the sum of following reactions? NO2(g) + NO2(g) ⇌ N2O4(g) N2O4(g) + CO(g) ⇌ NO(g) + NO2(g) + CO2(g)

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

In which direction does the following equilibrium shift when the gas mixture is compressed? Explain using Le Châtelier’s principle and in terms of forward and reverse reaction rates.          2 C(s) + O2(g) ⇌ 2 CO(g)