Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? 0 □ 0 0 0

Analyze the components of a voltaic electrochemical cell. A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Hg2+(aq) + Cu(s)→ Hg(I) + Cu²+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: + + Enter the reaction that takes place at the cathode. Include state symbols: + + In the external circuit, electrons migrate to v the Hg+ electrode from v the Cu electrode. In the salt bridge, anions migrate to the Cu compartment [from v) the Hg compartment.

Try Again Your answer is incorrect. Suppose the galvanic cell sketched below is powered by the following reaction: Ni(s)+ SnSO4(aq) → NiSO4(aq) + Sn(s) E1 S1 Write a balanced equation for the half-reaction that happens at the cathode of this cell. E2 Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? S2 2+ Sn (aq) + 2e Sn (s) 2+ Ni (s) → Ni²+ (aq) + 2e Nielectrode Snelectrode ロ→ロ 0,0,... X Ś

Use line notation to represent each electrochemical cell below a.  2Ag+(aq)+Pb(s)→2 Ag(s)+Pb2+(aq) b.  2ClO2(g)+2 I−(aq)→2 ClO2−(aq)+I2(s) c.  O2(g)+4 H+(aq)+2 Zn(s)→2 H2O(l)+2 Zn2+(aq)

In the following cell, write the half reaction that takes place at the anode and the half reaction that takes place at the cathode.

A galvanic cell is powered by the following redox reaction: 2+ 2 Cu²+ (aq) + H₂(g) + 2OH¯(aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 □ 0 E = v + 2 Cu (aq) + 2 H₂O(1) ロ→ X Ś

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.

signs a galvanic cell that uses these two half-reactions: half-reaction 2 H₂O(1)+2e H₂(g) + 2OH(aq) 3+ 2+ Fe³+ (aq)+e → Fe²+ (aq) 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 written. A chem standard reduction potential E-0.83 V red E 'red = +0.771 V 2H₂O(1) + 2e → H₂(g) + 2OH(aq) 2+ 3+ Fe → Fe (aq) + e 7 ロ→ロ e X x10 Ś ?

A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential Exed half-reaction 2 H2O(1)+2e → H2(g)+2OH (aq) Ε red -0.83 V 2+ Zn(aq)+2e →>> Zn(s) E = = -0.763 V 'red Answer the following questions about this cell.