Calculate AG and K at 25°C for the reactions. a. 7H₂O + 2 Cr³+ + 3 Cl₂ ⇒ Cr₂O7²- + 6 Cl¯ + 14H+ εº KJ AGⓇ = K = cell = 0.03 V

Use the data in Table 16.1 (or Appendix L) to calculate the equilibrium constant K at 25 °C for the following reaction. Mg(s) + Ni2+ (aq)→ Mg²+ (aq) + Ni(s) 0.0592 V log K E = n A

What is the standard free energy (in kJ/mol) and the value of the equilibrium constant, K, for the reaction at 300 K? 3Br2(l) + 2MnO2(s) + 4H2O(l) --> 6Br-(aq) + 2MnO4-(aq) + 8H+(aq)

The free energy change for the following reaction at 25 °C, when [Fe²*] = 1.18 M and [Cr³3+] = 8.62×10-3 M, is -186 kJ: 3FE2+(1.18 M) +2Cr(s)- →3F€(s) + 2C1³*(8.62×10-3 M) AG = -186 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?

What is the equilibrium constant for the following reaction at 25 °C? Round your answer to 1 decimal place. Cu(s) + 2Ag (aq) ⇒ Cu²+ (aq) + 2 Ag (s) Note: Reference the Standard reduction potentials at 25 °C table for additional information. K = x10 X S

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11. Consider the following reaction and its AG-AGo at 25.00 °C 2Ag(aq)+Cu(s) 2Ag(s)+Cu (aq) AG =-88660 J/mol a. Calculate the standard cell potential, E, for the reaction. b. Calculate the equilibrium constant, K, for the reaction.

11. Consider the following reaction and its AG-AG• at 25.00 °C. 12 Coeside 2Ag*(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG =-88660 J/mol a. Calculate the standard cell potential, Ecellº, for the reaction. b. Calculate the equilibrium constant, K, for the reaction. Wtoxided what is reduced? CLEAREY

The free energy change for the following reaction at 25 °C, when [H*] = 1.11 M and [Sn2+] = 1.21x10-3 M, is -43.9 %3D kJ: 2H*(1.11 M) + Sn(s) H2(g) + Sn2+(1.21x10-3 M) AG = -43.9 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction v forward reverse

Consider the cell below at standard conditions: Zn(s) | Zn 2+ (aq) || Fe 2+ (aq) | Fe(s)Calculate the value of ΔG° for the reaction that occurs if the value of E° cell = 0.32 V for this cell.