3. For the following reaction at equilibrium, AgBr < Ag+' 2+ Br'-1 what will be the effect on the solubility of the solid with the following changes: a. Addition of NaBr b. Addition of K2S c. Addition of AgNO3 d. Addition of CuCH3COO 4. For the following reaction at equilibrium, BaSO → Ba+2 + SO4-2? what will be the effect on the solubility of the solid with the following changes: a. Addition of Ca3(PO4) 2 b. Addition of BaCl c. Addition of Au2(SO4) 3 d. Addition of Li2CO3

Consider the general reaction below. X₂(g) + 2Y₂(g) = 2XY₂(g) K 3.9 x 10-8 @ 298 K - 0.50 M X2 and Y2 were added to a sealed vessel. Calculate the equilibrium concentrations of the components. What is the equilibrium concentration of XY2? [XY₂] = [?] x 10²] M Coefficient (green) Exponent (yellow) Enter

The equilibrium constant, K. for the following reaction is 7.00x10-$ at 673 K. NH,I(3)ENH3(3) + HI(E) Calculate the equilibrium concentration of HI when 0.521 moles of NH,I(s) are introduced into a 1.00 L vessel at 673 K. [HI] = M

When determining the equilibrium concentrations for the reaction AB(g) A(g) + B(g) [A][B] [AB] a simplifying assumption can be used under certain conditions to avoid solving a quadratic equation. Ke Kc = [AB]-x [AB] Classify each situation by whether the simplifying assumption can be used or whether the quadratic formula is required. Simplifying assumption can be used [AB] = 0.00178 M. Kc = 9.91 x 107 [AB]=0.0353 M, K, 3.67 x 10 Answer Bank [AB]=0.484 M, K, 8.18 x 10 Quadratic formula required [AB] 0.176 M. K=144 x 10¹ [AB]=0.0160 M, K - 7.46 x 10

Which of the following will disturb the system below that is at equilibrium? NHSH(s) NH3(g) + H2S(g) Choose one or more: Addition of ammonia Addition of hydrogen sulfide Addition of ammonium hydrogen sulfide Removal of ammonium hydrogen sulfide

Consider the reaction. А(аq) — 3 В(аq) K. = 2.15 x 10-6 at 500 K If a 4.80 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] =

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Write the equilibrium expressions for the following given reactions. a. Br2      +      2HI   -------------->   I2 + 2HBr b. 2NaHCO3(s)   -------------------->   Na2CO3(s) + CO2(g)  +   H2O(g)   1. Bromine monochloride (BrCl) decomposes to form bromine and chlorine:                         2BrCl(g)     ------->  Br2(g)        +     Cl2(g) At a certain temperature, the equilibrium constant for the reaction is 11.1. A sample of pure BrCl is placed in a 1.0 L container and allowed to decompose. At equilibrium, the reaction mixture contains 4.0 mol Cl2. What are the equilibrium concentrations of Br2 and BrCl?   2. Iodine molecules react reversibly with iodide ions to produce triiodide ions.          I2(aq)           +       I-(aq)    ---------->   I3(aq) If a liter of solution prepared from 1.00x10-3  mol of I2  and  1.00x10-3 mol of the strong KI contains 6.61x10-4 mol of iodine at eq., what is the eq. constant for the reaction? Establish an ICE chart.

A. Using the Le Chatelier's principle, predict the shift in the direction of the equilibrium position and changes that will be observed (e.g. color) in each of the following equilibria when the indicated condition is applied.| 1. Ifheat is added to a phase change equation at equilibrium from solid to liquid, which way will the reaction proceed? 2. In this reaction: H2Om = H2O how could conditions be manipulated to create more H2Qa? 3. Which side is heat on in this reaction (photosynthesis): 6COX + 6H2O@= C¢H12O620) + 60z) 4. Heat + Co+Ca+ 4 Claq) = COC4 ²- caq) when the equilibrium mixture is cooled. (exothermic) pink colorless blue 5. Fet) 6SCNa) - Fe(SCN)6 *w when Fe³+ is added to the equilibrium mixture. brown colorless red