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7.mmmlu5 pts.) A galvanic cell generates an electrochemical potential of 2.418 Volts, using 3 equivalents of...
A galvanic cell generates an electrochemical potential of 2.418 Volts, using 3 equivalents of electrons. The Gibb’s free energy is: (a) 233.3 KJ/mole (b) -128.9 KJ/mole (c) -699.8 KJ/mole (d) 128.9 KJ/mole
A galvanic cell generates an electrochemical potential of 2.418 Volts, using 3 equivalents of electrons. The Gibb’s free energy is: (a) 233.3 KJ/mole (b) -128.9 KJ/mole (c) -699.8 KJ/mole (d) 128.9 KJ/mole
2 pts Question 2 Calculate the cell potential for the galvanic cell (in volts) in which the following reaction occurs at 25.0°C, given than [Ti2] = 1.7 M and [Au3]-0.463 M. Standard reduction potentials can be found here . 3TY + 2Au) 3Tie)+2Au Note: Pay attention to the number of electrons transferred. Do not include units in your final answer Report your answer to two places after the decimal.
Calculate the cell potential for the galvanic cell (in volts) in which the following reaction occurs at 25.0∘C, given than [Ti2+] = 1.972 M and [Au3+] = 1.589 M. Standard reduction potentials can be found here (Links to an external site.). Note: Pay attention to the number of electrons transferred. Do not include units in your final answer. Report your answer to two places after the decimal.
Calculate the potential (in volts) for the voltaic (or galvanic) cell indicated at 25degreeC. Ga/G^3+ (10^-6 M) || Ag^+ (10^-4 M)/Ag 1.29 V 0.97 V 1.45 V 1.21 V 1.37 V
Consider a galvanic electrochemical cell constructed using Cr/Cr3* and Zn/Zn2+ at 25 °C. The following half-reactions are provided for each metal: Cr3+ (aq) + 3 e → Cr(s) Eºred = -0.744 V Zna*(aq) + 2 e Zn(s) Eºred = -0.763 V What is the standard cell potential for this cell?
Question 22 An electrochemical cell transfers 2 moles of electrons per mole of reactant and has potential (E9) = -0.93V Calculate the values of AGº for this cell in kJ Question 20 3 pts The pH of household ammonia is 11.9. What is the concentration of ammonia, NH, in units of molarity? Kb of NH3 is 1.76X 10 5. Show your work in part 2
Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V which half reaction takes place at the anode which is the standar cell potential write the balance equation for the overall reaction in acidic sol What is the cell potential for this cell at 25 °C when [Zn²⁺] =...
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An electrochemical reaction occurring in a galvanic cell is expressed using the standard cell notation: Zn(s) Zn2+ (aq) || Ag (aq) | Ag(s) The standard reduction potentials for the half-cell reactions are as follows: Zn2+(aq) + 2e_? Zn(s) E o=-0.76 V Ag (a)eAg(s) E +0.80 V Which of the following statements is correct regarding this electrochemical cell? A. Agt is reduced at the cathode; Zn is oxidized at the anode. B. Edell = +1.56 V...
3: Measuring cell potentia 1: Cathode Anode Measured EMF (volts) EMF calculated from Table 1 (volts) 1.562 Absolute error (volts) -0.002 Ag+ | Zn? Zn2+ +1.56 Mg 2+ +3.17 3.169 0.001 -0.002 3. Cuzt +0.46 0.462 4. Agt Agt 20 Mg 2+ Cuar Mght + 1.61 1.607 0.003 5. 24 r 110 0 3. Czt +2.71 2.207 0.003 Calculations: Calculations will continue on to the next page. Electrochemical Cells Post-Lab Questions: 1. Using the values from your simulation data: (a)...