DATASHEET EXPI KINETICS TO THERMODYNAMICS PART 1: EQUILIBRIUM: Ag (aq) + Fe2(aq) = Ag(s) + Fe(aq) Species AH, S AG, kJ mol-¹ JK-1 kJ mol-1 Ag (aq) 73.45 77.11 Fe2+(aq) -87.9 -113.4 -84.94 Ag(s) 42.6 Fe (aq) -47.69 1. Activation energy for forward reaction: 2. Activation energy for reverse reaction: 4. AS 3. AH 6. E° 5. AG

The below reaction was found to have AH = -3606 kJ mol-1 and AS = 33 J mol- K-1. What is AG for this reaction at 100.2 °C? 90,(g) + 2CH;CHCH,(g) – 6CO,(g) + 6H2O(g) Oa. -3618 kJ mol-1 Ob. -3609 kJ mol-1 Oc. -15927 kJ mol-1 Od. -3573 kJ mol-1 Oe. -3594 kJ mol-1

For the reaction 2 A(aq) <---> B(aq) + C(aq), the standard free enthalpy variation is 1.43 kJ at 25oC. The initial concentration of A is 0.541 M, the initial concentration of B is 0.343 M, and the initial concentration of C is 0.267 M. At equilibrium (we are still at 25oC), what will be the concentration of A( aq) (in mol/L)?

Use the following redox reactions and their corresponding ΔE° values:           Co(s) + Pb2+(aq) ⟶ Co2+(aq) + Pb(s)                  ΔE° = +0.15 V          Zn(s) + Co2+(aq) ⟶ Zn2+(aq) + Co(s)                  ΔE° = +0.48 V  Which one of these chemical species is the strongest oxidizing agent? Group of answer choices Pb2+(aq) Zn(s) Co(s) Insufficient information to answer this question. Co2+(aq)

The equilibrium constant Kc for C + CO2 <=> 2CO is 1.9 at 1000 K and 0.133 at 298K. Is the reaction endothermic or exothermic?

Carbon dioxide dissolves in water to form carbonic acid. Estimate the thermodynamic equilibrium constant for this reaction using the AG; values in the table. Substance AG; (kJ/mol) H,CO, (aq) -616.1 H,O(1) -237.1 CO,(g) -394.4 K = Carbonic acid then ionizes in water (K = 4.5 x 10-7). Ignoring K2, estimate K for the overall process by which CO, and H,O form H* and HCO,. K = What is the pressure of CO, in equilibrium with carbonated water at 25 °C and pH = 4.78? Роо, atm

R = 8.314 mol-K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕ - (E) · In(Q) ΔΕ. 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 M²+ (aq) + 2 e¯ H2 (g) + 2 OH¯ (aq) - 0.828 G (s) - 1.245 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. Calculate A E°. cell for this galvanic cell given the reference information given at the top of the quiz. Report your answer with 3 decimal places. You do not need to report units with your answer.

Calculate the equilibrium constant of the reaction Zn (k) + Fe²+ (aq) Fe (k) at 25 °C. E°(Zn²+ | Zn)= -0.76 V E°(Fe²+| Fe)= - 0.44 V ==> Zn²+(aq) +

Calculate K for the following reaction 2 Fe2+ (aq) +  Zr (s) ⟶ 2 Fe(s) + Zr4+ (aq) Zr4+(aq) + 4 e- ⟶ Zr(s); Eo = -1.539 VFe2+(aq) + 2 e- ⟶ Fe(s) Eo = -0.447 V   Group of answer choices 7.80x1036 2.79x1018 no correct answer 6.08x1073 2.39x107