The measured voltage of a cell in which the following reaction occurs is 0.29 V at 25 °C:
H2(g, 1.0 atm) + AgCl (s) ---> 2H+ (aq, pH = ?) + Ag(s) +Cl- (aq, 1.0M)
Calculate the pH of the cell above.
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The measured voltage of a cell in which the following reaction occurs is 0.29 V at...
The measured voltage of a cell in which the following reaction occurs is .96V. Calculate the pH of the H+ (aq) solution The measured voltage of a cell in which the following reaction occurs is 0.96 V H20g, l 0 atm) t Ag (aq, 1.0 M) 2H'(aq, pH 2Ag(s) Calculate the pl l of the H'(aq) solution b 5.4 c. 14.9
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this is the complete question (no more info) Determine the voltage (V) of the following cell at 25°C: Zn(s) | Zn2+(aq, 0.37 M) || Cl-laq, 0.75 M) C12(g, 0.750 atm)| Pt Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Hg2Cl2(s) + 2e --> 2Hg(l) + 2Cl(aq); E° = +0.27 V AgCl(s) + e --> Ag(s) + Cl (aq); E° = +0.22 V Ni2+(aq) + 2e --> Ni(s); E° =...
For the cell shown, the measured cell potential, ?cell, is −0.3629 V at 25 °C. Pt(s) | H2(g,0.899 atm) | H+(aq,? M) || Cd2+(aq,1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, ?o, are 2H+(aq)+2e−⟶H2(g)?o=0.00 V Cd2+(aq)+2e−⟶Cd(s)?o=−0.403 V Calculate the H+ concentration. [H+]=
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Test IV (Electrochemistry) 2018 Fall What is the oxidation number for the Which of the following is true concerning a galvanic cell? (A) Oxidation occurs at the anode and is 1. 8. underlined manganese in Mn04 (A)-8 (8)-2 (C)-1 (D)4 (E) 7 where anions move towards where anions move towards where cations move towards where anions move towards where anions move towards 2. When balancing the below half-reaction in acidic solutionelectrons are added to the (B) Oxidation occurs at the...