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Question 7 6 pts (25) The standard cell potential (Eºcell) of voltaic cellis +1.34 V. Calculate...
6 pts Question 7 (25) The standard cell potential (Eºcell) of voltaic cell is +1.10 V. Calculate the value of AGⓇ (kJ/mol) for the voltaic cell if 2 electrons are transferred between two half cells. -388 -212 +388 -24.3 +212
Question 6 0.5 pts Use tabulated half-cell potentials (found in appendix IV-D) to calculate Eºcell and then calculate AGºrxn for the following reaction at 25 °C. 2Fe3+ (aq) + 3Sn(s) Fe(s) + 3Sn2(aq) Hint: the standard potential of Fe3+ + 3e - Fe(s) is -0.036 and the standard potential of Sn2+ + 2e → Sn(s) is -0.140. AG° = -5 kJ/mol AG° = -10 kJ/mol AG° = -20 kJ/mol AG° = -30 kJ/mol AG° = -60 kJ/mol
Question 25 (4 points) The standard cell potential (Eºcell) of the reaction below is +1.73 V. The value of AG for the reaction is _____ kJ 3Ni (s) + 2 Au?+ (aq) + 3 Ni2+ (aq) + 2 Au(s) O +5.00x102 O +1.00x103 2140 0-1.00x103 0-5.00x102
Calculate ∆Go for the voltaic cell shown above.
n= moles of electrons transferred
F= 96500 Coulomb (charge on one mol of electrons)
Use the units kJ in your answer.
salt bridge Use these half-cell potentials: Cr2O72- (aq) + 14 H+ + 6e 2 Cr3+ (aq) + 7 H20 (1) O=1.36 Cl2 (9) + 2e → 2 C1 =1.33 Calculate AGº for the voltaic cell shown above. n= moles of electrons transferred F= 96500 Coulomb (charge on one mol of electrons)...
53-54
53) The standard cell potential (E®cell) of the reaction below is -0.55 V. The value of AGº for the reaction is J/mol. 12 (s) + 2Br- (aq) → 21- (aq) + Br2 (1) A) 0.55 B) 5.5 x 10-6 C) 1.1 x 105 D) 0.54 E) none of the above 54) The standard cell potential (Eºcell) of the reaction below is +1.34 V. The value of AGº for the reaction is kJ/mol 3 Cu (s) + 2 MnO4- (aq)...
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2 pts) a. Use the standard half-cell potentials listed below to calculate the standard cell potential (Eºcell) for 3 Sn(s) + 2 Fe* (aq) - 3 Sn2+ (aq) + 2 Fe(s) Sn 2(aq) + 2 e -Sn (s) E = -0.14 V Fe3+ (aq) + 3 e Fe(s) E° = -0.036 V A) -0.176 V B)-0.104 V C) +0.104 V D) +0.176 V b. Write...
Voltaic cells chemistry
please help with A-C, H and I.
3. A voltaic cell is built from two half-cells using the reduction reactions given below: Sn 2(aq) → Sn(s); Eredn = -0.14 V Cr20;2(aq) → Cr+ (aq) Eredin = 1.33 V a) Write the balanced cathode half reaction in acidic medium: (show work step by step and box your answer) b) Write the balanced anode half reaction and box your answer: c) Write the balanced overall cell reaction and box...
Use tabulated half-cell potentials (found in appendix IV-D) to calculate Eºcell and then calculate AGºrxn for the following reaction at 25 °C. 2Fe3+ (aq) + 3Sn(s) → 2Fe(s) + 3Sn2+ (aq) Hint: the standard potential of Fe3+ + 3e + Fe(s) is -0.036 and the standard potential of Sn2+ + 2e → Sn(s) is -0.140. AG° = -5 kJ/mol AG° = -10 kJ/mol AG° = -20 kJ/mol AG° = -30 kJ/mol
> Question 8 6 pts (Q6) The standard emf (Eºcell) for the cell using the overall cell reaction below is +2.20 V: 2Al(s) + 312 (s) 2A13+ (aq) + 61° (aq) Calculate reaction quotient "Q" when (A13+) - 0.35 M and [1 ] -0.15 M. 7.3 x 10 1.1x10 14x100 0.010 2.51
how
do I solve this?
1. Use the Nernst equation to calculate the standard cell potential for a voltaic cell of a Sn electrode in 0.10M Sn2(a) in one half-cell and Al in 0.10M AP) in the other. (EPe Eaode- Emode 1.52 V, Show your work. Hint: Check E values of the reduction haif reactions. Write the one with more negative E as oxidation half reaction (change the sign); ensure that equal number of electrons are exchanged ie. electrons cancel,...