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.
show the work D Question 21 An electrochemical cell is designated by the following shorthand notation:...
A. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 7.45×10-4 atm, the Cl- concentration is 1.21M, and the Cr3+ concentration is 1.37M ? 3Cl2(g) + 2Cr(s)6Cl-(aq) + 2Cr3+(aq) Answer: _____ V The cell reaction as written above is spontaneous for the concentrations given: ____ (true/false) B. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following...
help with these please
Write the cell notation for an electrochemical cell consisting of an anode where Al () is oxidized to AP+ (aq) and a cathode where Pb2+ (aq) is reduced to Pb (s). Assume all aqueous solutions have a concentration of 1 mol/L. Write the cell notation for an electrochemical cell consisting of an anode where Sn (s) is oxidized to Sn2+ (aq) and a cathode where H(aq) is reduced to H2 (g) at a platinum electrode. Assume...
Sketch a diagram of a galvanic cell represented by the following shorthand notation: Pb(s)|Pb2+ (aq)||Br2(1), Br (aq)|Pt(s) Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. e e → Group 1 2Br - Group 3 (anode) Pb2+ Salt bridge NaNO, Group 3 (cathode) Br2 NO3- Group 2 Na+ Group 2 Group 2 Pb Group 2 Group 2 Pt
Exercise 19.49 Use line notation to represent the electrochemical cells for each of the following overall redox reactions. Part A 2Ag+ (aq) + Pb(s) +2Ag(s) + PbP (o) O Ag(s) Ag+ (aq)||Pb2+ (aq) Pb(6) O Ag+ (aq) Ag(0) Pb(s)[Pb (4) O Pb2+ (aq)|Pb()||Ag()|Ag (og) O Pb(s)|Pb2+ (aq)||Ag+ (aq)|A6(*) Submit Request Answer Part B 2010 (8) +21 (aq) +2010, (4) +10) O Pt()CIO; () CIO,()||()T()Ps) Pt(s) C10(e) C10, (w) (0) (0) Pt(s) O POT" (aq) (||C10(e)C10; ()Pt(s) OPt()LOT ()||CO, (w) CIO,()PC)...
Complete the half-reactions for the cell shown, and show the shorthand notation for the cell. The electrode on the left is the anode, and the one on the right is the cathode. Anode half-reaction: РЫ Ag Pb(s) + 2 C1PCI () + 2e- Cathode half-reaction: AgCl(s) 2 AgCl(s) + 2e- Ag(s) + 2 C1- PbCI,() KCl(aq) KCl(aq) Shorthand notation: PbCl(s) Pb(s) Cl(aq) Cl(aq) Agcis) Ag(s) Answer Bank 2 AgCl(s) Pb(s) Cl(aq) AgCl(s) 2 Ag(s) PbCl () Ag(s) Incorrect
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2pressure is 2.71×10-4 atm, the F- concentration is 1.43M, and the Pb2+ concentration is 1.33M? F2(g) + Pb(s) ---> 2F-(aq) + Pb2+(aq) The cell reaction as written above is spontaneous for the concentrations given: True or False What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2pressure...
II Complete the half-reactions for the cell shown, and show the shorthand notation for the cell. The electrode on the left is the anode, and the one on the right is the cathode. 0 |Anode half-reaction: OD PbCl, (s) Pb(s) +201 – Cathode half-reaction: 2.AgCI() 2€ - PbCl,(s) KCl(aq) [ 285(0) AgCl(s) KCl(aq) 2 AgCl(s) Shorthand notation: Ag(s) | Pb(s) PbCl,(s) C1- (aq)] [c1-(aq)] | AgCl(s)) | 2 Ag(s) Answer Bank 2498) Ag(e) PbCly(@) Pb(8) 2.AgCI() CI+(ag) AgCl(s)
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)
calculate ecell for the following electrochemical cell at 25 C. Pt(s)| H2 (g,1.00 atm) | H+ (aq, 1.00 M) || (Pb2+ (aq, 0.150 M) | Pb (s) Pb^2+(aq) + 2e- ---> Pb (s) Eo=-0.126 V 2H^+ (aq) + 2e- ---> H2 (g) Eo=0.00 V Thank you!
For the electrochemical cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) | Zn2+(aq) || Ni2+(aq) | Ni(s) Zn(s) → Zn2+(aq) + 2 e- o Zn2+(aq) + 2 e- → Zn(s) + Ni(s) → Ni2+(aq) + 2 e- Ni2+(aq) + 2 e- → Ni(s)