Formation constant and Gibbs free energy For the complex formation reaction where Mis any metal and L is any ligand, - [ML2]+ M+ + 2L = Kr is the formation constant for the complex at equilibrium and AG is the Gibbs free energy change for the reaction at equilibrium. The formation constant (K) can be related to the Gibbs free energy change (AG°) for a reaction by the equation AG = RT In Kf where T is the temperature in kelvins and R is the gas constant equal to 8.314 J K. mol. The complex formation is generally a spontaneous process; thus, the Gibbs free energy change is negative. Part B Calculate the formation constant for the formation of [Cu(en) (H2O)4 from (Cu(H20)6]+, given that AG° is -60.1kJ - mol at 298 K

Formation constant and Gibbs free energy For the complex formation reaction where Mis any metal and L is any ligand, - [ML2]+ M+ + 2L = Kr is the formation constant for the complex at equilibrium and AG is the Gibbs free energy change for the reaction at equilibrium. The formation constant (K) can be related to the Gibbs free energy change (AG°) for a reaction by the equation AG = RT In Kf where T is the temperature in kelvins and R is the gas constant equal to 8.314 J K. mol. The complex formation is generally a spontaneous process; thus, the Gibbs free energy change is negative. Part B Calculate the formation constant for the formation of [Cu(en) (H2O)4 from (Cu(H20)6]+, given that AG° is -60.1kJ - mol at 298 K

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The fraction of sites bound on the particular macromolecule is 0.53 at a ligand concentration of 0.01992 mol/L. The equilibrium constant of the ligand binding reaction is 460. Determine the Hill coefficient.
4. Consider the following reaction: [ZnCl4]² +4 OH → [Zn(OH)4]² +4 CI If the reaction is spontaneous, then which of the following is true? (A) Chloride is a more labile ligand than hydroxide in zinc complexes (B) Hydroxide is a more labile ligand than chloride in zinc complexes (C) Chloride is a more inert ligand than hydroxide in zinc complexes (D) Hydroxide and chloride are equally labile in zinc complexes
Which of the following is responsible for the chelate effect exhibited by multidentate ligands? Only one ΔGo > 0 ΔSo < 0 Formation of an octahedral complex ΔSo > 0 Formation of 1:1 Metal-Ligand complex ΔG < 0
Name the following metal complexes or complex ions: formula name [Fe(OH), (en),] [V(CN),(NH,).] TiF ?
31 For the aqueous [Ni(CN)4] complex K₁=2.00 × 10³¹ at 25 °C. .2+ Suppose equal volumes of 0.0052M Ni (NO3), solution and 1.0M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Ni²+ ion. Round your answer to 2 significant digits. M x10 × Ś
Use the thermodynamic data below to compute the average bond enthalpy of the metal-ligand bonds in [Cu(NH3)4]2+(aq). Species ΔfH0kJ/mol S0J/mol/K NH3(aq) -80.29 111.3 Cu2+(aq) 64.77 -99.6 [Cu(NH3)4]2+(aq) -348.5 273.6 Include 3 significant figures
Take into consideration metal Z(III) ion which is able to form octahedral complexes with elther fluoride or cyanide ions, What can be said about the colors of the complexes formed when one complex ion absorbs at 650 nm while the other at 430 nm?
1c
A) Using a cobalt (III) ion as the central metal atom, and with chloride ions (Cl-) and ammonia (NH3) molecules as the ligands, draw both isomers of the coordination complex that will exhibit fac/mer isomerism. B) Using a platinum (II) ion as the central metal atom, with chloride ions and ammonia molecules as the ligands, draw both isomers of the coordination complex that will exhibit cis/trans isomerism. Platinum (II) forms four coordinate bonds.
In water, the Fe3+ ion exists as Fe(H2O)63+. Fe(H2O)63+ is a complex ion in which the ligands are water molecules. The high positive charge on the Fe3+ ion makes the coordinated water acidic, and Fe(H2O)63+ behaves as an acid, as described by the following reaction. Fe(H2O)63+ (aq) -> H+ (aq) + Fe(H2O)5(OH)2+ (aq) A solution is prepared by dissolving 0.0500 mole of Fe2(SO4)3 in water and diluting to yield 1.00 L of solution. A)- What is the molar concentration of sulfate ion in the solution. B)- Experiments show an osmotic pressure of 6.73 atm for this solution at 25 oC. Calculate the molarity of solutes in the solution. C)- What is the molar concentration of Fe(H2O)5(OH)2+ in the solution? (use your answers from A and B to find this)
The complex [Fe(CO)6]+2 exhibits π-acceptor behavior. Using ligand field theory, draw the molecular orbital diagram mixing the d-orbitals on the metal and the molecular orbitals on the ligands and fill in the available electrons. What is the nature of the t2g orbitals that are part of Δo, bonding, antibonding, or non-bonding? Explain your answer. Is this molecule high spin or low spin? Explain your answer.
Chemistry In the reaction between aqueous,cobalt(II) chloride with ammonia, the only complex to be formed is the hexaammine species [Co(NH,). The six stepwise stability constants, K, -Kg, corresponding to this ligand substitution reaction at 298K, are given below. K, = 1.5 x 10 K, = 1.3 x 10 K, = 3.6 x 10' K, = 7.4 x 10° K = 0.4 K = 0.07 Fill in the blanks to provide a balanced equation representing Step 1 of this reaction. NH, - H,0 Calculate the overall stability constant B6 for this reaction. B6 = x 10A Calculate the value of AG° (298K) for the formation of [Co((NH,)". R = 8.314 J'K'moi' -1 AG° = kJmol Select whether the following statements are true, false, or cannot be determined (ND). a. Formation of [Co(NH,),1 is a spontaneous process . AS is expected to be positive for this transformation . At low concentrations of ammonia, ligand substitution does not occur 1. The value for K, indicates that the equilibrium mixture contains more products than reactants 2+ e. Based on the value…