The free energy change for the following reaction at 25 °C, when [Pb2+] 6.68x10-3 M, is -368 k): = 1.13 M and [Cr3+] = %3D 3P62+(1.13 M) + 2Cr(s)3Pb(s) + 2Cr3+(6.68x10-3 M) AG = -368 kJ What is the cell potential for the reaction as written under these conditions? Answer: Would this reaction be spontaneous in the forward or the reverse direction? forward reverse

The free energy change for the following reaction at 25 °C, when [Pb2+] 6.68x10-3 M, is -368 k): = 1.13 M and [Cr3+] = %3D 3P62+(1.13 M) + 2Cr(s)3Pb(s) + 2Cr3+(6.68x10-3 M) AG = -368 kJ What is the cell potential for the reaction as written under these conditions? Answer: Would this reaction be spontaneous in the forward or the reverse direction? forward reverse

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

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 [Ag*] = 1.20 M and [Cu2+] = 8.38x10-3 M, is -101 kJ: 2Ag*(1.20 M) + Cu(s)2Ag(s) + Cu2+(8.38x10-3 M) AG = -101 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
None
Given the following reactions: Anode: NO3- + 2H+ + e- --> NO2 + H2O Cathode: 2H+ + 2e- --> H2 Redox: 2NO2(g) + 2 H2O (I) --> 2NO3-(aq) + 2H+(aq) + H2(g) Conditions: [0.15 atm] [0.18 atm] [0.1 M] [0.67 atm] Find the pH, if E = - 0.70 V. %3D
Kk68.
The free energy change for the following reaction at 25 °C, when [Zn²+] = 2.66×10³ M and [Cr³*] = 1.12 M, is 28.3 kJ: 3Zn2*(2.66x10-3 M) + 2Cr(s)→3Zn(s) + 2Cr³†(1.12 M) AG = 28.3 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?
Oxidation of lactate by cytochrome C (represented as cytochrome C (Fe3 +)) to pyruvate is an important biological reaction.Below are the reduction reactions and standard reduction potentials (E °) at pH = 7 and 25 ° C.Pyruvate + 2H + + 2e- = Lactate - (E ° = -0.185 V)Cytochrome C (Fe3 +) + e - = Cytochrome C (Fe2 +) (E ° = 0.254 V) Considering the Gibss free energy and Nernst equations, calculate the following equilibrium ratio (K) at 25 ° C, pH = 7.
Calculate ΔG° and K (at 298K) for this reaction: 2H2S(g) + SO2(g) ↔ 3S(s) + 2H2O(g)
Calculate the cell voltage at 25°C for this cell when [H+] = [HSO4–] = 4.5 M. At 25°C, E° = 2.04 V for the lead-acid battery. For this reaction, ∆H° = –315.9 kJ and ∆S° = 263.5 J/mole K. Calculate E° at –20° C and Ecell when [H+] = [HSO4–] = 4.5 M.
Calculate the theoretical cell potential of the following cells. If the cell is short-circuited, indicate the direction of the spontaneous cell reaction. Zn/Zn²+ (0.1000 M) // Co²+(5.87 x 104 M)/ Co Ez2+ = -0.763V E Co2+ = -0.277V O +0.419 V spontaneous reaction +0.422 V spontaneous reaction O +0.421 V spontaneous reaction +0.420 V spontaneous reaction
4-ele The free energy change for the following reaction at 25 °C, when [Cr³"]= 4.83×103 M and [Hg²+]= 1.13 M, is 937 kJ: 2Cr*(4.83×103 M) + 3Hg(1)– 2+ →2Cr(s) + 3Hg²*(1.13 M) AG = 937 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 forward reverse
Consider the following reaction at 298K. Cu²* (aq) + Fe²* (aq) Cu* (aq) + Fe* (aq) Which of the following statements are correct? Choose all that apply. On-1 mol electrons OK>1 AG° <0 E° cell 0 The reaction is reactant-favored.