Given the equilibria and AG° values below: A B+C B+D=E FE+C What is the AGº for the reaction A + D = F? a. 4 kJ/mol b. 8 kJ/mol c. 12 kJ/mol d. 24 kJ/mol AG° = 6 kJ/mol AG° 4 kJ/mol = AG° = 2 kJ/mol
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- Given that K₁ and K₂ are the respective equilibrium constants for the two reactions ? MnO₂ (s) + 2H₂(g) Mn(s) + 2H₂O(1) CO₂(g) + H₂(g) ? CO(g) + H₂O(1) K₁ = 40.8 K₂= 3.08x10-4 Determine the equilibrium constant for the reaction Mn(s) + 2 CO₂(g) ? MnO₂ (s) + 2 CO(g) K =11. The equilibrium constant for the reaction: AgBr(s) = Ag*(aq) + Br" (aq) is the solubility product constant, Ksp = 7.7 x 10 -13 at 25°C. %3D Calculate AG for the reaction when [Ag *] = 1.0 x 10 -2 M and [Br -] = 1.0 x 10-3 M. %3D Is the reaction spontaneous or nonspontaneous at these concentrations?The reaction CO₂(g) + C(s) = 2CO(g) has a K₁= 5.78 at 1200 K. a. An for the reaction is bns b. Calculate Kc for the reaction. una
- The enthalpy of vaporization of CH3OH is 6.40 kJ/mol. What is the entropy change for vaporization of 20.0 g CH3OH if the boiling point of it is 40.0 0C? (atomic weight in amu: C 12.00; H 1.00; O 16.00) OA. 5.0 /k O B. 12.8 J/K Oc. 20.5 J/K 18.5 J/K OD. 100 J/K OE.R = 8.314 mol·K F = 96, 485 moi AG = AG° + RT · In(Q) ΔΕΔΕ-().In(Q) RT Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e 2 H20 (1) 1.229 - Z2 (s) + 2 e 3+ (aq) + 3 e 2Z (aq) 0.426 → A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e H2 (g) + 2 OH (aq) - 0.828 G (s) - 1.245 > M2+ (aq) + 2 e M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. If the A 3+ (aq) solution is diluted to 0.100 M and the G<* (aq) solution is diluted to 2+ 0.500 M, what is the initial value of Q under these new conditions? Report your answer with the correct significant figures.2. Consider the equilibrium A(g) 2 B(g) +C(g) One mole of A is placed in a vessel at 298 K and allowed to come to equilibrium at a total pressure of 3.0 bar. An analysis of the contents of the vessel at equilibrium reveals that the partial pressure of A is twice that of B. a) Calculate Kp b) Calculate Kc Calculate AG (1 M standard state) *
- 6-Consider the first ionization of sulfurous acid: H2SO3(aq) → H*(aq) + HSO3 (aq) Certain related thermodynamic data are provided below: H2SO3(aq) H* (aq) HSO3 (aq) ----- Hf kcal/mole -145.5 -151.9 S° cal/mole K 56 26 (a) Calculate the value of AG° at 25°C for the ionization reaction. (b) Calculate the value of K at 25°C for the ionization reaction. (c) Account for the signs of AS° and AH° for the ionization reaction in terms of the molecules and ions present.Given each value, determine whether the starting material or product is favored at equilibrium.a. Keq = 0.5b. ?G° = -100 kJ/molc. ?H° = 8.0 kJ/mold. Keq = 16e. ?G° = 2.0 kJ/molf. ?H° = 200 kJ/molg. ?S° = 8 J/(K · mol)h. ?S° = -8 J/(K · mol)Given the following values of equilibrium constants: [Ag(NH,)2]* = Ag* (aq) + 2NH3(aq) K 6.3 x 10-5 Ag,SO3(s) = 2Ag* (ag) + SO?-(aq) K= 1.50 x 10-14 What is the value of the equilibrium constant for the following reaction? Ag, SO3 (s) + 4NH3 (aq) = 2[Ag(NH,)2]+ +SO (aq)
- Consider the following equilibrium reaction: Cu+2 (aq) + 2 Ag (s) = Cu (s) + 2 Ag*1 (aq) What is the Kc expression? Select one: [Ag+1]² [Cut2] O a. Ke [Ag+1] O b. K. = [Cut2] [Cut2] [Ag+1]² ,+2 O c. Ke = [Ag+1]*[Cu] [Cu+2][Ag]? O d. Ke [Cu+2] [Ag+1] O e. KcCalculate AG and K at 25°C for the reactions. 7H20 +2 Cr** +3 Cl2 Cr2 0,2- +6 Cl +14H+ = 0.03 V a. Ecell AG° = kJ K = Cu2+ (aq)+Ba(s) Ba2+ (ag) + Cu(s) e = 3.24 V b. AG = kJ K = Cl2 (g) + 2 Br (ag) = Br2 (g) +2 Cl¯(aq) e° = 0.27 V c. AG kJ K = d. 3H20(1) +5 IO, (ag)+2 Mn²+ (aq) 5103 (aq) + 2 MnO4 (aq) + 6H (aq) Eell = 0.09 V AG kJ K =9. (10 marks) The equilibrium constant (KP) at 25 °C is 3.2 x 10-10 for the reaction: 2 Cr³+ (aq) + Pb(s) 2 Cr2+(aq) + Pb2+(aq). a. (3 marks) A 12.9 g coil of lead wire is placed in a flask containing 200.0 mL of 0.500 mol/L Cr3+(aq) at this temperature. Find the concentration of each ion once the reaction has come to equilibrium at this temperature.