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O pts Question 10 You must show your work to receive points for the following question. It doesnt matter if you answer true or false. Points will be adjusted based on work shown. Bonus: for up to five extra points show the work to answer the following question Consider a galvanic cell that uses the reaction: 2 Ag+laq) + Sn(s) --> 2 Ag(s) + Sn2+(aq) Calculate the cell potential at 25C for a cell that has the following ion concentrations:...
You must show your work to receive points for the following question. It doesnt matter if you answer true or false. Points will be adjusted based on work shown. What is rust? What causes it to form (explain with regards to anodic and cathodic regions)? What are two methods employed to prevent its formation? True False
4 pts Question 8 You must show your work to receive points for the following question. It doesnt matter if you answer true or false. Points will be adjusted based on work shown. What is rust? What causes it to form (explain with regards to anodic and cathodic regions)? What are two methods employed to prevent its formation: True Fale
Post Lab Questions: To receive full credit, you must SHOW ALL YOUR WORK!! Use the table of reduction half reactions to answer the following Post-Lab questions: Table 3. Example reduction Reduction Potential Chart half reactions. The easiest to Ce+(aq) + 3e - Ce3+ (aq) reduce is at the top. The more Au3+ (aq) + 3e Au(s) difficult to reduce is at the bottom. Cl2(g) + 2e 2CH(ag) Ag+ (aq) + e- Ag(s) Fe3+ (aq) + e- Fe2+ (aq) AgCl(s) +...
please show all work. thank you 4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
Co (s) | Co2+ (aq) || Au3+ (aq) | Au (s) Q3\ For the previous cell, determine the concentration of the cobalt ion when a cell voltage of 1.76 V is obtained using a 0.761 M gold (III) nitrate solution. Q4\ Calculate the free energy for the nonstandard cell in the previous problem. Show all work. Be mindful of signs, sig figs, and units Q5\ Consider a galvanic cell consisting of the following two redox couples: Sn2+ (aq, 0.010 M)...
HELP NEED ANSWERED TODAY BY 11:50PM!!! Part A Write balanced equation for the anode of the following galvanic cell Fe(s)|Fe2+(aq)||O2(g)|H+(aq),H2O(l)|Pt(s) Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Write balanced equation for the cathode of the following galvanic cell Fe(s)|Fe2+(aq)||O2(g)|H+(aq),H2O(l)|Pt(s) Express your answer as a chemical equation. Identify all of the phases in your answer. Part C Write balanced equation for overall cell reactions of the following galvanic cell Fe(s)|Fe2+(aq)||O2(g)|H+(aq),H2O(l)|Pt(s) Express...
Question 15 3 pts Consider a palvanic cell that uses the reaction 2 A* (aq) + Sn(s) 2 Ac(s) + Snag) Calculate the potential at 25°C for acell that has the following ion concentrations:(Ac)-0,010 M. (Sn?") - 0.020 M.(Refer to a table of standard reduction potentials.) 0.93V O 0.94V o 101V O 0.87V
Please show all work! Thanks! Calculate the equilibrium constants of the following reactions at 25°C from standard potential data (a) Sn(s) Sn+(aq)2 Sn2+(aq) 1.54e-10 (b) Sn(s) + 2 AgCl(s)SnCl2(aq) + 2 Ag(s) 2.04e18
Please show all work step by step and final answer. Cell Potential at Equilibrium For a single galvanic cell based on the (unbalanced) reaction: Ag+ (aq) + Zn(s) = Zn2+(aq) + Ag(s) What is the cell potential when the cell reaches equilibrium? Submit Answer Tries 0/5