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The standard reduction potentials for Cu^2+/Cu and Zn^2+/Zn are given below: Cu^2+(aq) + 2e^rightarrow Cu(s) +0.34 V Zn^2+(aq) + 2^e- rightarrow Zn(s) -0.76 V a. If a strip of copper metal is placed into a solution of ZnS0_4(aq), will a reaction occur? Explain why and write the net ionic equation for the reaction, if any. b. If a strip of zinc metal is placed into a solution of CuSO_4(aq), will a reaction occur? Explain why and write the net ionic equation for the reaction, if any c. Complete the voltaic cell set-up below assuming it is a Cu-Zn cell utilizing Cu and Zn solid strips, and CuSO_4 (aq) and ZnSO_4, (aq) solutions in the beakers. Draw and label all missing components. Include the direction of electron flow and the direction at which ions flow from a K_2SO_4(aq) salt bridge.
The standard reduction potentials for Cu^2+/Cu and Zn^2+/Zn are given below: Cu^2+(aq) + 2e^rightarrow Cu(s) +0.34 V Zn^2+(aq) + 2^e- rightarrow Zn(s) -0.76 V a. If a strip of copper metal is placed into a solution of ZnS0_4(aq), will a reaction occur? Explain why and write the net ionic equation for the reaction, if any. b. If a strip of zinc metal is placed into a solution of CuSO_4(aq), will a reaction occur? Explain why and write the net ionic equation for the reaction, if any c. Complete the voltaic cell set-up below assuming it is a Cu-Zn cell utilizing Cu and Zn solid strips, and CuSO_4 (aq) and ZnSO_4, (aq) solutions in the beakers. Draw and label all missing components. Include the direction of electron flow and the direction at which ions flow from a K_2SO_4(aq) salt bridge.
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Irving HeathcoteLv2
26 Jan 2019
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