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- Given the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.For the following reaction: A(g) + 3 B(g) ⇌ C(g) + 2 D(g) Calculate the magnitude of Kp (don't report the units) assuming the following composition at equilibrium: PA = 0.61 bar PB = 0.926 bar PC = 0.24 bar PD = 0.779 barConsider the decomposition of a metal oxide to its elements, where M represents a generic metal. Substance ΔG°f(kJ/mol) M2O3(s) −8.00 M(s) 0 O2(g) 0 M2O3(s)↽−−⇀ 2M(s)+32O2(g)M2O3(s)↽−−⇀ 2M(s)+32O2(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? Δ?∘rxn=ΔGrxn°= kJ/molkJ/mol What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? ?=K= What is the equilibrium pressure of O2(g) over M(s) at 298 K? ?O2=PO2= atm
- The solubility product constant (Ksp) for the following reaction is 5.61x10-9. What is the Free Energy of this reaction in kJ at 298 K? BaCO3(s) ↔ Ba2+(aq) + CO32-(aq)Using any data you can find in the ALEKS Data resource, calculate the quilibrium constant K at 25.0°C for the following reaction. Fe2O3(s)+ 3H2(g)→ 2Fe(s)+ 3H2O(l) Round your answer to 2 significant digits. delta G of Fe2O3=-742.2 kj/mol h2=0 Fe=0 H20=-237.1kj/molReaction KspKsp ΔH°ΔH° ΔS°ΔS° FeCO3(s)⇄Fe2+(aq)+CO32−(aq)FeCO3(s)⇄Fe2+(aq)+CO32−(aq) 3×10−113×10−11 <0<0 >0>0 MnCO3(s)⇄Mn2+(aq)+CO32−(aq)MnCO3(s)⇄Mn2+(aq)+CO32−(aq) 2×10−112×10−11 <0<0 >0 The table above lists the equilibrium constants and changes in thermodynamic properties for the dissolution of FeCO3 and MnCO3 at 25°C. The two-particle diagrams below represent saturated solutions of each compound at equilibrium. (see attached image) a.) The particle diagrams best represent that ΔH°<0ΔH°<0 because the ions from both compounds are solvated by water molecules. b.) The particle diagrams best represent that ΔH°<0ΔH°<0 because both compounds produce about the same amount of CO32−CO32− ions from the dissolution. c.) The particle diagrams best represent that ΔS°>0ΔS°>0 because both compounds produce a very small amount of ions from the dissolution. d.) The particle diagrams best represent that the molar solubility is greater for…
- The equilibrium constant for the reaction AgBr(s) Ag+(aq) + Br– (aq) is the solubility product constant, Ksp = 7.7 × 10–13 at 25°C. Calculate ΔG for the reaction when [Ag+] = 1.0 × 10–2 M and [Br–] = 1.0 × 10–3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? (R = 8.314 J/K • mol) A. ΔG = –97.5 kJ/mol, nonspontaneous B. ΔG = 40.6 kJ/mol, nonspontaneous C. ΔG = 97.5 kJ/mol, spontaneous D. ΔG = 69.1 kJ/mol, nonspontaneous E. ΔG = –69.1 kJ/mol, spontaneous1. The solubility product constant for Ag3PO4 is 2.8 x10^-18. What is the solubility of silver ion in the solution? a. 5.37 x10 ^-5 b. 1.79 x10^-5 c. 2.8 x10^-15 d. 3.6 x10^-13 e. None of the above 2. Determine the equilibrium constant Kp at 25 C for the reaction: 2NO(g) + O2(g) ---> 2NO2 (g) delta G degree Rxn = -69.7 kJ/mol a. 1.65x10^12 b. 8.28 x10^-2 c. 2.6 d. 13.4 e. 6.07 x10^-13Determine the equilibrium constant for the system N2O4 2NO2 at 25°C. The concentrations are shown here: [N2O4] = 2.32 ´ 10-2 M, [NO2] = 1.41 ´ 10-2 M.
- The solubility product, Ksp, for the following solubility equilibrium at 25oC is 1.1 x 10-10. BaSO4(s)<--> Ba+2(aq) + SO4-2(aq) Calculate the standard free energy change for this equilibrium at this temperature. Group of answer choices 0.470 kJ/mol 56.8 kJ/mol 5.61 kJ/mol 4.77 kJ/molThe generic metal A forms in an insoluble salt Ab(s) and a complex AC5(aq) The equilibrium concentration in a solution of AC5 were found to be [A] = .100M, [C]=.0120M and [AC5]=.100M. Determine the formation canstant ,Kf of AC5 Kf=? The solubility of AB(s) in a 1.000M solution of C(aq) is found to be .143M What is the Ksp of AB? Ksp=?The equilibrium constant for the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) is Kc=1.3×10−2 @ 1000 K. Calculate Kc for 2NOBr(g)⇌2NO(g)+Br2(g). Express your answer using two significant figures.
