Question

The formation of CoCl42- from Co2+ and Cl- is endothermic. Are the color changes that accompany...

The formation of CoCl42- from Co2+ and Cl- is endothermic. Are the color changes that accompany heating and cooling of the equilibrium mixture in agreement with Le Chatelier's principle? Explain

Homework Answers

Answer #1

The formation of CoCl42- from Co2+ and Cl- is endothermic. Yes, the color changes that accompany heating and cooling of the equilibrium mixture is in agreement with Le Chatelier's principle.

[Co(HO)6]+ +4Cl- + heat → [Co(Cl)4]2- + 6H2O

Pink color                             Blue color

According to Le Chatelier’s principle, on heating the reaction or adding more Cl-, will drive the reaction to the right side. On cooing the reaction or removing Cl- will drive the reaction to the left side.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
PbCl2 (s) ==== Pb2+ (aq) + 2 Cl- (aq) Record your observations for the following changes...
PbCl2 (s) ==== Pb2+ (aq) + 2 Cl- (aq) Record your observations for the following changes and explain each in term of Le Chatelier’s principle. Write net ionic equations for the reactions which occur. 1. Heating the PbCl2 mixture. 2. Addition 1.0 M Na2CO3 to the clear liquid. 3. Reaction with 1.0 M HNO3. 4. Reaction with Na2S.
What would you expect to observe if you added a saturated NaCl solution to a pink...
What would you expect to observe if you added a saturated NaCl solution to a pink [CoCl4]2-/[Co(H2O)6]2+ equilibrium mixture? Compare this predicted effect to the actual effect (color changes to blue) and account for your answer using Le Chatelier's Principle.
Re-write the chemical reaction for the CoCl42- complex. You may refer to the experimental procedure. CoCl42-...
Re-write the chemical reaction for the CoCl42- complex. You may refer to the experimental procedure. CoCl42- (aq) + 6H2O (l) Û 4Cl- + Co(H2O)62+ (aq) + energy (purple/blue)                            (pink) A completed data table #3. Change to the Reaction Drops added Visual observation Shift in the reaction (to the products, to reactants, or no change) Test tube 1: CoCl2 + water 4 To begin, the solution was a purple/blue color. There were no solids in the solution. Although, after the reaction...
B. SATURATED AMMONIUM CHLORIDE. NH4CL + HCL 1. what is the evidence for a shift in...
B. SATURATED AMMONIUM CHLORIDE. NH4CL + HCL 1. what is the evidence for a shift in equilibrium? 2. which ion caused the equilibrium to shift? 3. In which direction did the equilibrium shift? C. IRON(III) CHLORIDE PLUS POTASSIUM THIOCYANATE a. stock solution b. stock solution +FeCl3 c. stock solution +KSCN d. stock solution + AgNO3 +KSCN e. stock solution +AfNO3+ FeCl3 1. 1. What is the evidence for a shift in equillibrium when iron(iii) chloride is added to the stock...
Chemical Equilibrium: Le Chatelier’s Principle. 1. Add 0.5 mL of 0.1 M FeCl3(aq) to 0.5 mL...
Chemical Equilibrium: Le Chatelier’s Principle. 1. Add 0.5 mL of 0.1 M FeCl3(aq) to 0.5 mL of 0.1 M KSCN(aq), and then add 15 mL of distilled water. To a 2-mL portion of this mixture, add 1 mL of 0.1 M KSCN(aq). Observe any difference in the color from the original solution and explain your observations. Because you are combining equal volumes of equal concentrations, and because they combine in a 1 to 6 mole ratio, Fe3+(aq) should be in...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are equal b)the value of the equilibrium constant is 1 c)all chemical reactions have ceased d)the rate constants of the forward and reverse reactions are equal e)the limiting reagent has been consumed 2)The equilibrium-constant expression depends on the ________ of the reaction. a) stoichiometry b) mechanism c) the quantities of reactants and products initially present d) temperature e) stoichiometry and mechanism 3)Given the following reaction...
ASAP FOR ALL QUESTIONS ABOUT THE Le Chatelier’s Principle LAB Procedure : I ) NaCl (s)...
ASAP FOR ALL QUESTIONS ABOUT THE Le Chatelier’s Principle LAB Procedure : I ) NaCl (s)   ßà   Na+ (aq)   + Cl- (aq)          *Add few drops of conc. HCl to 2 to 3 mL of saturated NaCl solution. II ) NH4Cl(s) ßà NH4+ (aq) + Cl-(aq)          *Add few drops of conc. HCl to 2 to 3 mL of saturated NH4Cl solution. III ) Fe+3(aq) + SCN-(aq) ßà Fe(SCN)+2(aq)          Prepare a stock solution by mixing 2mL each of 0.1M...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this experiment. What is the relationship between concentration and ionization? Explain the reason for this relationship 2.) Explain hydrolysis, i.e, what types of molecules undergo hydrolysis (be specific) and show equations for reactions of acid, base, and salt hydrolysis not used as examples in the introduction to this experiment 3.) In Part C: Hydrolysis of Salts, you will calibrate the pH probe prior to testing...
      MK Restaurant: Branding of Thai-Style Hotpot The restaurant industry is one of the most...
      MK Restaurant: Branding of Thai-Style Hotpot The restaurant industry is one of the most competitive in Thailand. With a large number of players ranging from restaurants in five-star hotels, global fast-food chains to small stalls along the streets and everything in between, the Thais are spoiled for choice. In addition, as the world becomes globalized, consumers are familiar with international dishes and would not hesitate to try new offerings from the other side of the globe. As a...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT