i am confuses how to calculate Ecell where non-standard condition for this question For the following...
For the following questions: a)Calculate ??????for the spontaneous reaction b)Write the overall cell equation c)Write the cell notation for the cell d)Calculate ??? e)Calculate ?????where non-standard conditions are stated 1)cell is made from the ??3+,(??,0.10?)|??and the ???4-(??,0.25?)|??2+,(??,1.50?)half cells, where pH is 1.67 at 298 K(no need to calculate ???for this Q) 2)A cell is made from the ??|??+,(??,0.010?)and the ???4-(??,2.0?)|???2half cells, where pH is 0 at 298 K(no need to calculate ???for this Q)
QUESTION 27 Calculate Ecell under non-standard conditions for the following electrochemical cell: Pt(s)| FeCl2 (aq, 0.150 M), FeCl3 (aq, 0.050 M) || Cl2 (9, 1 atm), NaCl (aq, 0.075 M) | Pt (s) -1.60 V 0.72 v 0.69 V -1.79 V 0.62 V none of these
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...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
Use the standard reduction potential values from your chemistry data sheet to answer this question. The following electrochemical cell has a potential of Ecell = 0.322 V at 298 K: Sn (s) | Sn2+ (aq) (0.025 M) || M2+ (aq) (0.010 M), M+ (aq) (0.025 M) | Pt(s) Where M2+and M+ are ions of an unknown metal. First, determine the standard potential of the anode (EA°) -0.138 V +0.138 V 0.00 V None of the above What is the value...
Given the measured cell potential, Ecell, is-0.3583 V at 25 °C in the following cell, calculate the Ht concentration Pt (s)|H2lg, 0.795 atm)lH (aq, ? M)l|Cd2 (aq, 1.00 M)|Cd (s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are as follows. 2H+(aq) + 2e- H2(g) E0.00 V E-0.403 V ? 2 + Number H0.21
Calculate Ecell for the following electrochemical cell at 25 degreeC Pt(s) | H2(g, 1.00 atm) | H+ (aq, 1.00 M) || Pb2+(aq, 0.150 M) | Pb(s) given the following standard reduction potentials. Pb2+(aq) + 2 e– --> Pb(s) Edegree = –0.126 V 2 H+ (aq) + 2 e– --> H2(g) Edegree = 0.000 V (Please show the steps)
Name SHOW ALL WORK. NO CREDIT UNLESS ALL WORK IS SHOWN. ROUNDING/SIG FIG ERRORS WILL BE PENALIZED. 1. Parts a-j of this question refer to the following cell at 298 K. Complete the diagram of the following voltaic cell: Silver and iron electrodes, aqueous Silver nitrate, aqueous iron (UI) nitrate, potassium nitrate salt bridge. Fe3+ (aq) + 3e → Fe (s) Ag (aq) + e - Ag(s) E° -0.040 V Eº= 0.795 V a. Identify the electrodes as Anode or...