We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Consider the voltaic cell at 25 °C 21. Zn(s) | Zn2 (aq, 1.0 x 10 2...
Question 2 (1 point) Consider the following voltaic (galvanic) cell: Zn(s) | 0.010 mol/L Zn2+ (aq) || 1.0 mol/L Cu2+(aq) | Cu(s) What is the predicted cell potential when this cell is operated? 1.04 V 1.10 V 0.76 V 0.34 V 1.16 V
Consider a voltaic cell where the anode half-reaction is Zn(s) → Zn2+(aq) + 2 e− and the cathode half-reaction is Sn2+(aq) + 2 e– → Sn(s). What is the concentration of Sn2+ if Zn2+ is 2.5 × 10−3 M and the cell emf is 0.660 V? The standard reduction potentials are given below Zn+2(aq) + 2 e− → Zn(s) E∘red == −0.76 V Sn2+(aq) + 2 e– → Sn(s) E∘red −0.136 V
Hello is the answer 1.041 or 1.16 point) Consider the following voltaic (galvanic) cell: Zn(s) 0.010 mol/L Zn2+ (aq) || 1.0 mol/L Cu2+(aq) | Cu(s) What is the predicted cell potential when this cell is operated? 1.04 V 1.10 V 0.76 V 0.34 V 1.16 V
A voltaic cell represented by the following cell diagram has Ecell= 1.409 V . Zn(s)|Zn2+(1.00M)||Ag+(saturated Ag2X)|Ag(s) What must be the Ksp of Ag2X? Use the following standard electrode potentials: Zn2+(aq) + 2e- →Zn(s) E° = -0.764 V Ag+(aq) + e- →Ag(s) E° = 0.799 V To enter your answer, multiply your Ksp by 1x109 then enter it to 2 decimal places.
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.80 molL−1 and 0.130 molL−1, respectively. Zn2+(aq)+2e−→Zn(s)E∘=−0.76V Ni2+(aq)+2e−→Ni(s)E∘=−0.23V A) What is the cell potential when the concentration of Ni2+ has fallen to 0.600 molL−1? B) What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V?
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.60molL−1 and 0.130 molL−1, respectively. Zn2+(aq)+2e−→Zn(s)E∘=−0.76V Ni2+(aq)+2e−→Ni(s)E∘=−0.23V Part A What is the initial cell potential? Part B What is the cell potential when the concentration of Ni2+ has fallen to 0.600 molL−1? Part C What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V?
Please include solutions, thank you. Consider the voltaic cell: Zn(s) + Cd2+(aq) → Zn2+ (aq) + Cd(s). (Eºcell = 0.36V) operating at 319.351 K. If (conc. Cd2+) = 0.411 and (conc. Zn2+) = 1.101, calculate the Ecell (volts).
Consider the voltaic cell and reduction half potentials: Zn(s) | Zn 2+(aq) (0.100 M) || Ni2+(aq) (1.50 M) | Ni(s) Zn 2+ (aq)/Zn (s) E o = - 0.760 V Ni2+ (aq)/Ni (s) E o = - 0.230 V a) Sketch the voltaic cell represented with the above line notation. Label the anode and cathode and indicate the half-reactions occurring at each electrode and the species present in each solution. Also indicate the direction of electron flow (3 marks). b)...
1.A voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s) + Ni2+(aq) Zn2+(aq) + Ni(s) 2.A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+(aq) + Cr(s) 3 Ce3+(aq) + Cr3+(aq) We were unable to transcribe this imageA voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s) + Ni2+(aq) → Zn2+ (aq) + Ni(s) (a) What is the emf of this cell under standard...
1) A particular voltaic cell operates on the reaction Zn(s) + Cl2(g) → Zn2+ (aq) + 2C1- has a cell potential of 0.853 V. Calculate the maximum electrical work generated when 15.0 g of zinc metal is consumed.