A strip of copper is placed in a 1 M solution of copper nitrate and a strip of silver is placed in a 1 M solution of silver nitrate.The two metal strips are connected to a voltmeter by wires and a salt bridge connects the solutions.The following standard reduction potentials apply: Ag⁺(aq) + e^- $\to$ Ag(s)
$\varepsilon$ ^$\circ$ =+0.80 V
Cu²⁺(aq) + 2e^- $\to$ Cu(s)
$\varepsilon$ ^$\circ$ = +0.34 V
Which of the following statements is false?

Question

A strip of copper is placed in a 1 M solution of copper nitrate and a strip of silver is placed in a 1 M solution of silver nitrate.The two metal strips are connected to a voltmeter by wires and a salt bridge connects the solutions.The following standard reduction potentials apply: Ag⁺(aq) + e^-

\to

Ag(s)

\varepsilon

^$\circ$ =+0.80 V
Cu²⁺(aq) + 2e^-

\to

Cu(s)

\varepsilon

^$\circ$ = +0.34 V
Which of the following statements is false?

Quizplus · Accepted Answer

The false statement is C because in a galvanic cell, ions move through the salt bridge to maintain electrical neutrality, not to directly react with the other electrode. Silver ions do not move through the salt bridge to the copper half-cell; instead, negative ions typically move from the silver half-cell to the copper half-cell to balance the charge as copper ions are plated onto the copper electrode and silver ions are deposited onto the silver electrode from their respective solutions.

A Strip of Copper Is Placed in a 1 M →\to→

A Strip of Copper Is Placed in a 1 M $\to$