Complete the two reduction half reactions for the cell shown at the right, and show the...
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
Attempt 2 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. Pb Anode half-reaction: Ag() +20 = A Ag(s) + 2e Cathode half-reaction: Agla + 2e Ag(s) + 2 CI PCL KC) AgCl) KCMag) Shorthand notation: Pb(s) PECI() Cr(4) Cl(aq) ACC) AC Answer Bank 2 AgCl) Cl(aq) Ag(s) 2 ARCO AgCl) PC1,() Pb(s)
Complete the half-reactions for the cell shown, and show the correct 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: +20H = D. +2 Cathode half-reaction: ********* 2 2 *****720H Shorthand notation: Cu(OH)2(s)- bcccc -C(OH)2(s) Answer Bank KOH(aq) CO(OH),(s) Co(s) KOH(aq) Cu(s) Cu(OH),(s)
Question 14 of 31) Complete the half-reactions for the cell shown, and show the correct 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: +2e Cathode half-reaction: 2 OH Shorthand notation: Shorthand notation: Answer Bank KOH(aq)) (Cu(OH)2(s)) (Ni(s) Ni(OH)2(s), cu(s) Attempt 3 Cu Ni Cu(OH)2(s) Ni(OH)2(s) KOH(aq) Attempt 3 for 0 Cu Ni Cu(OH)2(s)-- 9:31 PM 5/8/2019
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)
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential MnO2 (s) + 4H+ (aq) +2e−→ Mn+2 ( aq) +2H2O(l) =E0red+1.23V Cl2 (g) +2e−→ 2Cl− (aq) =E0red+1.359V Answer the following questions about this cell Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as...
5. A galvanic cell is constructed which uses the following half reactions. The initial concentration of each aqueous reactant and product is 0.100 M. H2O2(aq) + 2H"(aq) + 2e 2H2O() CIO-(aq) H2O(l) + 2Cl(aq) + 2OH(aq) a. Write the line notation for the cell. (5 pts) b. Write the net ionic equation for the cell reaction. (5 pts) c. Calculate the initial potential of the cell. (5 pts) Answer: d. Calculate the pH in the anode and cathode compartments after...
First fill in your half cell and cell reactions. F in standard cell potentials as you calculate them. Oxidation at the Anode: The black (.) lead is attached to the electrode, which is the source of electrons. Write the anode half reaction: Reduction at the Cathode: The red lead (+) is attached to the electrode. Write the cathode half reaction: E degree - V. Overall Cell Reaction (Net Ionic equation): Write the overall cell reaction (balance electrons and add together):...
Draw a functioning electrochemical cell that uses any two of the following half reactions shown below. Include a graphite electrode. Label the anode, cathode, direction of electron flow, direction of ALL ion/metals, and expected cell voltage. Write a balanced electrochemical reaction for your cell in neutral conditions).
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Ed=-0.763 V Zn²+(aq)+2e MnO2 (aq)+8H+ (aq)+5€ → Zn(s) → Mn²+ (aq)+4 ,00) E cd = +1.51 v Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is...