6. Analyze the GC traces from each of the reactions shown below. The GC parameters for each trace are identical: Br. NaOH DCM 3.20 min 3.81 min Br, NaOH DCM 1 2 4 1 2 3.20 min 2.82 min 2.82 min 3.20 min 3.81 min

For the reaction: PbCl2(s) Pb2+(aq) +2C11-(aq), what is Q* when 8.0 mL of 0.050 M lead nitrate is added to 14 mL of 0.031 M sodium chloride? Ksp of lead chloride is 1.6 x 10-5 M³. Hint given in general feedback *Recall: Q is compared to Ksp to determine whether a precipitate forms.

< Progress:0/9 groups Due Apr 18 at 11:55 PM Use the References to access important values if needed for this question. In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42-. Co2+(aq) is pink and CoCl42-(aq) is blue. ... At Low Temperature the pink color predominates. ... ... At High Temperature the blue color is strong. ... If we represent the equilibrium as:...Co2+(aq) + 4Cl-(aq) CoCl42-(aq)We can conclude that: fill in the blank 1 1. This reaction is:     A. Exothermic     B. Endothermic     C. Neutral     D. More information is needed to answer this question. fill in the blank 2 2. When the temperature is decreased the equilibrium constant, K:     A. Increases     B. Decreases     C. Remains the same     D. More information is needed to answer this question. fill in the blank 3 3. When the temperature is decreased the equilibrium concentration of Co2+:     A. Increases     B. Decreases…

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PAP Chemistr x G diagram show X PAP Chemistr x G Reactions that X EPAP Chemistr X PAP Chemistr X HAC Session Timer X Mp Rocking Whee X + b ar-2903012.agilixbuzz.com/student/135113422/activity/c412d902-b23e-4202-b813-76alf9f4c196 175% Reset Mastery Assess It_8 Enrique Solis PAP Chemistry-2903012-42100P-1... All changes saved 6. You have a very concentrated solution (12 M) of potassium chloride (KCI). You need it to be at the lowest concentration possible for the experiment you are about to conduct. The problem is you forgot to order lab supplies, so you only have 2 L of distilled water left. What would be the final concentration if you added the two 2 L of distilled water to the 0.5 L of 12 M KCI? 3.0 M 2.4 M 24 M 48 M

Kk.364.

For 2SO2 (g) + O2 (g) <-------> 2SO3 (g) Concentrations: [SO2]=0.20, [O2]=0.80, [SO3]= 0.43.  What is Kc for the reaction?

1. Write the dissociation reaction and solubility product constant expression for the following sparingly soluble salt. a. AgBr Ksp = 5.2 x 10-13 b. PbCl2 Ksp = 1.7 x 10-5 %3D 2. Determine the Molar Solubility of the following sparingly soluble salt in water. a. AgBr Ksp = 5.2 x 10-13 b. PBCI2 Ksp = 1.7 x 10-5 3. Express the solubility (S) in question #2 in g/L.

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How would the equilibrium be affected in regards to the value of Qc or Kc for each of the following conditions?: Fe3+ (aq) + SCN- (aq) ⇌ FeSCN2+ (aq) Adding KSCN (aq) Adding Fe(NO3) (aq) Adding NaF (s) Placing the solution into a hot water bath Placing the solution into an ice bath (To whom this may concern, Could you at least explain one as simply as possible so I'm able to understand the others enough to explain them myself? Thanks in anvance!)