we will investigate the equilibrium of cobalt chloride and explore the influences of concentration and temperature. An equilibrium exists between anhydrous cobalt chloride ([CoCl4]² and a hydrated form of cobalt ([Co(H₂O)]²+. Assume this reaction is taking place at 298 K. [Co(H₂O)6]²+ (aq) + 4 Cl(aq) = [CoCl4]² (aq) + 6H₂O(1) blue pink Kc = 1.7 X 10-³ Explain what happens to the equilibrium composition when hydrochloric acid (HCI) is added to the cobalt chloride equilibrium. Your explanation should refer to Q and K.

The equilibrium constant for the reaction                         2 KAl(OH)4(aq) + 4 H2SO4(aq)  ⇆ 2 KAl(SO4)2(s) + 8 H2O(l) at room temperature is 84.5. At equilibrium, the concentration of sulfuric acid (H2SO4) is 0.258M. What is the concentration of KAl(OH)4 (in moles/L)?

Try Again Check your chemical formulas. Write the equilibrium constant expression for this reaction: 2H (aq)+CO (aq) → H2CO3(aq) ☐ ☑ == D

Predict the equilibrium concentration of NH in the reaction described below (for which Kc = 1.210 at the reaction temperature) by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. = NHSH(s) NH¸(g) + H₂S(g) Using the data from your ICE Table (Part 1), construct the expression for the equilibrium constant, Kc. Each reaction participant must be represented by one tile. Do not combine terms. KC = II = 1.2 × 10-4 RESET [x] [2x] [2x]² [1.2 × 104+x] [1.2 × 104-x] [1.2 × 104 + 2x] [1.2 × 104 -2x] [1.2 × 10+ + x]² [1.2 × 10+ - x]² [1.2 × 10+ + 2x]² [1.2 × 104 -2x]²

Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes spontaneously but slowly. The decomposition reaction will proceed at a faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed reaction are: H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq) OO H₂O₂(aq) + Ol(aq) → H₂O(l) + O₂(g) +1-(aq) a. What is the net reaction? b. If 10.00 mL of H₂O₂ undergoes this reaction, what mass of oxygen is produced? c. If the reaction has an 85.5% yield, what mass of oxygen is actually produced?

Chapter 12 part 1 #12

The equilibrium constant for the chemical equation N,(g) + 3 H, (g) = 2 NH, (g) is Kp = 0.402 at 267 °C. Calculate the value of K. for the reaction at 267 °C. K. =

The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K. Calculate Ke for this reaction at this temperature. C PC15 (g) → PC13(g) + Cl₂ (9) Kc = ||

Most reaction do not go to completions. Equilibrium is established between the reactants and products. For the reaction of A with B to produce C and D, we can write the chemical equation as: аА + bв + сс + dD where + represents equilibrium between the reactants and products. The extent to which the reaction proceeds to product formation, at a given temperature, is given by the equilibrium constant, Kę. The equilibrium constant is written mathematically (for the above equation) as: [C[[D]* K. = [A]°[B]" where, a, b, c, and d are the stoichiometric coefficients from the balanced chemical equation and the brackets, [ ], indicate molar concentration. 1. For the following reaction: 2A + В + 3с calculate the equilibrium constant, K, if at equilibrium the concentration of A is 0.15M, the concentration of B is 0.20M, and the concentration of C is 0.10M.

Explain your reasoning, please. Thank you.