Co(NH3)4C1803]+ + 2H3O+ →1 [Co(NH3)5(H2O)]3+ + 2H2O + CO2 If the oxygen atoms of the coordinated carbonate were labeled with 180, where in the products the ? labeled oxygen will end up
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![Co(NH3)4C1803]+ + 2H3O+ →]
[Co(NH3)5(H2O)]3+ + 2H2O + CO2
If the oxygen atoms of the coordinated carbonate
were labeled with 180, where in the products the
? labeled oxygen will end up](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc6acd946-09df-4b82-9f8c-69805a9228cf%2Fd59d9ffa-5344-4bd1-851b-4ed3b5cd9cf8%2Ftwc58ph_processed.jpeg&w=3840&q=75)
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- [Co(H2O)6]2+ (aq) + 4 Cl-(aq )⇆ [CoCl4]2-(aq) + 6 H2O 3. Does the value of the equilibrium constant (K) for this reaction increase, decrease, or remain the same as the concentration of chloride increases? Explain your answer incorporating the definition of an equilibrium constant.COBALT COMPLEX: [CoCl4]2-(aq) + 6H2O(l) « [Co(H2O)6]2+(aq) + 4Cl-(aq) + Heat Blue Pink STEPS #- Solutions Observations 1-DISSOLVE COBALT COMPLEX PINK SOLUTION 2-SOLUTION PLUS HCl BLUE SOLUTION 3-ADD WATER PINK SOLUTION 4-HEAT SOLUTION BLUE SOLUTION According to the equilibrium equation, which ion(s) do you have when the solution dissolved? Explain how you know the identity of the ion(s) present. 2. Explain what happened when the HCl was added to the solution. 3. Explain what happened when the H2O was added to the solution. 4. Explain what happened when the solution was heated. Was the reaction exothermic or endothermic?[Co(H2O)6]2+ (aq) + 4 Cl-(aq )⇆ [CoCl4]2-(aq) + 6 H2O Explain why the addition of water changes the equilibrium position even though the concentration of water is essentially constant and normally not included in the equilibrium constant expression. What are two functions that water performs in this reaction?
- Co(NH3)4C1803]+ + 2H3O+ →1.20 [Co(NH3)5(H2O)]3+ + 2H2O + CO2 If the oxygen atoms of the coordinated carbonate were labeled with 180, where in the products the labeled oxygen will end up * ?Which statement is true regarding the following reaction? cis-Λ-[Co(en)2Cl2] + OH− --> cis-[Co(en)2Cl(OH)] + Cl− Group of answer choices At high OH- concentrations, the product complex is a Δ isomer. This reaction does not actually take place - instead of en ligands, there must be NH3 ligands. At low OH- concentrations, the product complex is a Δ isomer. The first step of this reaction mechanism is the dissociation of Cl-.2) [Co(NH3)4CO:]* + 2H3O* → [Co(NH:)s(H20)] + 2H20 + CO2 If the oxygen atoms of the coordinated carbonate were to be labeled with "0, where in the products the labeled oxygen will end up? Answer:
- Based upon the equilibrium reaction shown, what will happen in each case and why? [Co(H2O)6]2+ + 4 Cl- ⇄[CoCl4]-2+ 6 H2O a.)2 M HCl is added to the solution. b.)DI water is added to the solution. c.)If the solution turned blue upon heating in a 80°C water bath. d.)If the solution turned Pink upon immersion into a 0° water bath.[Co(H2O)6]2+ (aq) + 4 Cl-(aq )⇆ [CoCl4]2-(aq) + 6 H2O Is this reaction endothermic or exothermic?4. a. An equilibrium exists in solution between [Co(NH3)6]³+ + 3 en = [Co(en)3]³+ + 6 NH3 Which side of the equilibrium is favored?
- Consider the following reaction: [Cr(H2O)5(SCN)]2+ + Yn- --> [Cr(H2O)5Y](3-n)+ + SCN- Which statement is true if this reaction occurs via a dissociation mechanism? Group of answer choices Changing the incoming ligand, Yn-, will have a large effect on the rate constant. The first step of the mechanism is the addition of the Yn- ligand to form a 7-ccordinate intermediate, [Cr(H2O)5(SCN)Y](2-n)+ Changing the incoming ligand, Yn-, will have very little effect on the rate constant. It is impossible for this reaction to occur via a dissociation mechanism.1. Write the oxidation and reduction half equations of this reaction. Co(NO3)2.6H2O + 4NH3(aq) + (NH4)2CO3 + ½ H2O2 → [Co(NH3)4CO3]NO3 + NH4NO3 + 6H2O + NH4OH 2. Ali synthesized an octahedral complex with the formula, [Co(NH3)4CO3]Cl. - Draw the structure of this complex. Name it.Consider the following equation: [Ni(H2O)6]2+ + 6NH3 <----> [Ni(NH3)6]2+ +6H2O The effects of stress on this equilibrium can be monitored by changes in color. An equilibrium mixture is blue-green (indicating both products and reactants are present). a.) When the equilibrium mixture is heated, the color changes to bright green. Which direction has the reaction shifted? To the products, the reactants, or no shift? How did you determine this? Which is the exothermic direction of this reaction? Forward, reverse, or cannot tell? b.) When a few drops of concentrated NH3 are added to the equilibrium mixture, the solution turns deep blue. Which direction has the reaction shifted? To the products, the reactants, or no shift? How did you determine this? c.) Addition of concentrated HNO3 to the blue-green mixture will remove NH3 by reaction. What should happen to the color of the solution? Will it turn more blue, turn more green, or no change? Explain.