1811-cc1033tmodurl-08path-/ Mail e Edit View Favorites Tools Help 2 What is the

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1811-cc1033tmodurl-08path-/ Mail e Edit View Favorites Tools Help 2 What is the significance o... Amazon.com- Online Sh.. Office 365 Outlook Exchange oweredby Office 385 Download d Online Find ) Help U Give Feedback to Micros Print ID: A Consider an electrochemical cell with a zinc electrode immersed in 1.0 MZn?+ and a silver electrode immersed in 1.0 MAgt. Calculate e for this cell. a 0.04 V b. 1.56 V c. 1.56 V d. 0.04 V e none of these 13. 14. If a constant current of 5.0 amperes is passed through a cell containing Cr+ for 1.0 hour, how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51 996) a 62 10 a

Explanation / Answer

The more positive the Eo the greater is the tendency for the reaction to occur. In other words, Ag+ is a stronger oxidizing agent (gains electrons) than is Zn+2
Thus, the Zn half reaction must be reversed and the sign of Eo changed.
Zn === Zn+2 + 2e- +0.761
Ag+ + e- == Ag +0.80
Multiply the Ag+ equation by 2 so that the number of electrons gained equals
The number lost. Do NOT multiply the +0.80 by 2.

Zn === Zn+2 + 2e- +0.761
2Ag+ + 2e- == 2Ag +0.80

Zn + 2Ag+ == Zn+2 + 2Ag +1.561

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