Write a balanced chemical equation which corresponds to the following equilibriu

Question

Write a balanced chemical equation which corresponds to the following equilibrium constant expression. K = [Fe^3+][OH^-]^3 FeOH^2+(s) doubleheadarrow Fe^3+(aq) + OH^-(aq) 3 Fe^3+(aq) + 3 OH^-(aq) doubleheadarrow 3 Fe(OH) (aq) Fe(OH) (aq) doubleheadarrow Fe^3+(aq) + 3 OH^-(aq) Fe(OH) (s) doubleheadarrow Fe^3+(aq) + 3 OH^-(aq) Fe^3+(aq) + 3 OH^-(aq) doubleheadarrow 3 Fe(OH) (s) What is the relationship between K_p and K_c for the reaction below? CS_2(g) + 3 Cl_2(g) doubleheadarrow S_2Cl_2(g) + CCl_2(g) K_c = K_p/(RT)^2 K_q = (RT)^2/K_p K_q = (RT)^2 K_p K_c = (RT/K_p)^2 K_q = (K_p/RT)^2 Consider the reaction A(g) 2 B(g) where K_p = 5.0 at 25 degree C. If 0.50 mol A and 2.0 mol B are introduced into a 1.0 L flask at 25 degree C, what change in concentrations (if any) will occur in time? [A] will decrease and [B] decreases. [A] will decrease and [B] increases. [A] will increase and [B] increases. [A] will increase and [B] decreases. [A] and [B] remain unchanged If the reaction quotient, Q, is greater than K_p, then the chemical system has reached equilibrium. the temperature must be increased for the reaction to proceed in the forward direction. the reaction will proceed in the direction that results in fewer gas phase particles. the reaction will proceed to the right until equilibrium is established. the reaction will proceed to the left until equilibrium is established. The reaction below is studied at a high temperature. PCl_2(g) PCl_3(g) + Cl_2(g) At equilibrium, the partial pressures of the gases are as follows: PCl_5 = 1.8 times 10^-2 atm, PCl_3 = 5.6 times 10^-2 atm, and Cl_2 = 3.8 times 10^-4 atm. What is the value of K_p for the reaction? 3.8 times 10^-7 1.2 times 10^-3 3.1 8.5 times 10^2 2.6 times 10^6 At a given temperature, an equilibrium mixture contains the following concentrations of gases: [SO_3] = 0.054 M, [SO_2] = 0.0047 M, [O_2] = 0.58 M. What is the equilibrium constant, K_c, for the reaction below? 2 SO (g) doubleheadarrow 2 SO_2(g) + O_2(g) 4.4 times 10^-3 5.0 times 10^-2 11 2.0 times 10^2 2.3 times 10^2 We place 0.0774 mol N_2O_4(g) in a 1.00 L flask at a given temperature. After reaching equilibrium, the concentration of NO_2(g) is 0.0068 M. What is K_c for the reaction below? N_2O_4(g) doubleheadarrow 2 NO_2(g) 8.8 times 10^-5 5.9 times 10^-4 6.2 times 10^-4 7.2 times 10^-4 9.6 times 10^-2

Explanation / Answer

Option -d is the correct answer.

Fe(OH)2 (s) ------------->Fe3+(aq)+3OH- (aq)

The equilibrium constant K =[concentration of products]/[concentration of reactants]=[Fe3+]*[OH-]^3/[Fe(OH)2]

The [Fe(OH)2] is unity as the pure solid exerts no pressure on the system since any change in the solid concentration does not change the equilibrium constant

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