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Write equilibrium constant expressions for the following reactions in terms of concentration: (a) 2 CH C12(E)=...
Write the equilibrium constant expressions for the follow- ing reactions: (a) 2 CO(g) + O2(g) 2 2 CO2(8) (b) Mg(s) + HCl(aq) 2 MgCl2(aq) + H2(8) (c) HF(aq) + H2O(l) 2 H30+(aq) + F(aq) (d) S(s) + O2(8) 2 SO2(8) e 1 11
2) Write the equilibrium constant expressions for each of the following reactions. (For gas-phase reactions, write the Ke expression.) a) 2 NO(g) + O2(g) = 2 NO2(g) b) 4 Ag(s) + O2(g) + 2 Ag2O(S) c) CaCO3(s) + CO2(aq) + H2O(l) = Ca2+(aq) + 2 HCO3(aq) 3) a) Write the K, expressions for reactions a and b in problem 2. b) If the value of K for reaction a in problem 2 is 2.8 x 1011 at 200°C, what is...
Tutored Practice Problem 16.2.3 COUNTS TOWERS GUIDE Manipulate equilibrium constant expressions. The equilibrium constant for the following reaction is 15.5 at 396 °C. SO2(g) + Cl2(g)— SO2Cl2(g) K=15.5 at 396 °C Calculate the equilibrium constant for the following reactions at 396 °C. (a) SO2Cl2(E) SO2(E) + Cl2(e) K=[ (b) 2 SO2C12(g)— 2 SO2(g) + 2 C12(E) K= Check & Submit Answer Show Approach
1. Write equilibrium expressions for each of the following reactions (*Concentration of a solid is a constant) SICL(g) + 2H2 (g) Si(s) +4HCI(g) a. 2+ Zn(s) + Fe Zn (aq) + Fe(s) b. (aq) lculate the value of the equilibrium constant of the reaction of SO, and Wat e H2SO4 when the concentrations at equilibrium are as follows [SO] = 0 -0.480M H,O@ HSO + 40
More Equilibrium: Please write equilibrium expressions for the following reactions: 1. i. 2 SO2 (g) + O2 (g) 2 SO3 (g) il. NH4NOs (s) N2O (g) +2 H20 (g) i CaCO3 (s) + CaO (s) + CO2 (g) iv. HNO2 (aq) +H2O (I) HaO* (aq) + NO2 (aq) 2. Predict which way the equilibrium will shift for each of the following changes: CO (g) + H2 (g) C (s) H2O (g) + heat i. increase [H2O] ii. increase [C0] iii....
1. Write down the equilibrium constant expressions, Ke and K, for each of the following reactions: (a) H(g)Cl(g) 2 HCl(g) (b) 2 C(s)+O2(g) 2 CO(g Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 O(g) 3 0:(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O, and 0.060 mol of NO2 at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant Ke for the reaction? N2O4(g) 2 NO:(g)...
1. Write down the equilibrium constant expressions, K, and K for each of the following reactions: (a) H2(g)C(g) 2 HCl(g) (b) 2 C(s)+0(g) 2 COg Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 0,(g) 30,(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O and 0.060 mol of NO, at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant K, for the reaction? N,0,(g)2 NO(g) 3. Ammonium...
1. Write the equilibrium constant expressions (Kc) for the following reactions: (a) CO (g) + H2O (g) ⮂ CO2 (g) + H2 (g) (b) CH4 (g) + 2H2S (g) ⭢ CS2 (g) + 4H2 (g) (c) COCl2 (g) ⮂ Cl2 (g) + CO (g) (d) 2HI (g) ⮂ H2 (g) + I2 (g) (e) PCl3 + Cl2 (g) ⮂ PCl5 (g) (f) 2H2 (g) + O2 (g) ⮂ ...
1. Write down the equilibrium constant expressions for the following reactions: (a). 4 NO2(g) + O2(g) + 2 H2O(1) 44 HNO3(aq) (b). Zn(s) + Fe2+(aq) — Zn2+(aq) + Fe(s) H2O(1) (c). Mg(OH)2(s) — Mg2+(aq) + 2 OH (aq)
For each of the following reactions: (a) Write the Equilibrium expression (b) Calculate the Equilibrium Constant, Kc (c) Determine the DIRECTION of the reaction (d) Determine if the reaction is in Equilibrium (e) Determine the effect of INCREASING the temperature (f) Determine the effect of increasing the concentration of ONE of the reactants. (g) Determine the effect of increasing the volume of the container. (h) Determine the effect of increasing the Pressure in the container. Reaction 1: N204(g) 2NO2(g) Reaction...