Several values of K (the equilibrium constant) and AH (enthalpy change) are given. For each value, determine whether reactants or products are favored at equilibrium. Be sure to place all the values.
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- The Ka of HCHO2 is 1.8 x 10-4. Calculate the ΔGº (in kJ/mol) for the acid dissociation reaction at 25ºCWhat is the Ksp of Cr(OH)3 if its solubility is 1.3 x 10-6 g/L? (MM = 103.0 g/mol) 9.6 x 10-31 9.6 x 10-13 6.9 x 10-31 6.9 x 10-13Calculate the value of the equilibrium constant for each of the following reactions in aqueous solution. a) HC2H3O2 + OH- <--> C2H3O2- + H2O b) C2H3O2- + H+ <--> HC2H3O2 c)HCl + NaOH <--> NaCl + H2O and I need an actual value for Kc not just the Kc formula which I already know. thanks.
- Did you first add the H2O(l) on the right side of the equaton and then added the 2HO- on the left side and multiplied CIO2 on the left side by 2?The acid - dissociation constant (Ka) of chlorous acid (HCIO2) is 1.1 x 10-2 Calculate the concentrations of H+. CIO 2-, and HCIO2 at equilibrium if the initial concentration of HCIO2 is 0.0125 M1.For the aqueous reaction A + B à C + D, the equilibrium concentrations in moles per liter are [A] = 0.002, [B] = 0.005, [C] = 0.00004 [D] = 0.00025 i. What is the equilibrium constant Keq? ii. What is the dissociation constant pK? a. The partial pressure of gas A is 10 ppmv. It has a Henry’s constant for dissolution in water of KH = 0.02
- What is Kb for the equilibrium rreacton: CN- + H2O <=> HCN + OH- ? Ka value of 6.23 x10-10Given the following information: F1- (aq): ΔGf° = -276.48 kJ/mol Na1+ (aq): ΔGf° = -261.87 kJ/mol 2 Na (s) + F2 (g) → 2 NaF (aq) a) Find ΔG° for this reaction using the above numbers. b) Write the expression for Qeq. (Note that NaF is a strong electrolyte!) c) Find ΔG at 325.0 K for 0.01500 atm F2 and 3.065 M NaF.options for all: 1. Reactants. 2. Products.
- Given each value, determine whether the starting material or product isfavored at equilibrium.a.) Keq = 0.5b.) ΔGo = −100 kJ/molc.) ΔHo = 8.0 kJ/mold.) Keq = 16e.) ΔGo = 2.0 kJ/molf.) ΔHo = 200 kJ/molg.) ΔSo = 8 J/(K•mol)h.) ΔSo = −8 J/(K•mol)At 25oC, Ka for acid dissociation of lactic acid (HC3H5O3) is 1.0 x 10-4. Calculate ΔGo for the reaction HC3H5O3 (aq) + H2O(l) H3O+(aq) + C3H5O3-(aq)The following equilibrium concentrations were measured at 25 ∘C∘C:Lactic acid [C3H6O3]=9.64×10−2 M; [H+]=3.65×10−3 M;Lactate ion [C3H5O3−]=3.65×10−3 M. What is the concentration of lactic acid C3H6O3 if at equilibrium [C3H5O3−]=[H+]=1.07×10−2 M?