A voltaic cell is constructed based on the following reaction: Sn2* (aq) + Pb(s) + Sn (s) + Pb2* (aq) a) If the concentration of Sn2+* in the cathode half-cell is 1.00 M and the cell generates an emf of +0.22 V, what is the concentration of Pb2+ in the anode half-cell? b) If the anode half-cell contains [SO,²¯] = 1.00 M in equilibrium with PBSO4 (s), what is the Ksp of PbSO4?

A voltaic electrochemical cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. → Sn²*(aq) + Hg(1) 2+, Sn(s) + Hg²*(aq) · What is the reaction that takes place in the anode compartment? + + What is the reaction that takes place in the cathode compartment? + + In the external circuit, electrons migrate v the Hg²* electrode v the Sn electrode. In the salt bridge, anions migrate the Hg** compartment| v the Sn compartment.

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Br₂(1)+2e → 2 Br (aq) N₂(g) + 4H₂O()+4e N₂H₂(aq)+4 OH (aq) standard reduction potential E 'red E = red +1.065 V - 1.16 V

A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Cr(s) + 3FE3+(aq)Cr3+(aq) + 3F22+(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 v the Cr electrode v the Fe3+, Fe2+ electrode. Anions migrate v the salt bridge the Fe3+, Fe2+ compartment. Submit from proach Show Tutor Steps to