?Assume that you want to construct a voltaic cell that uses the following
Chapter 20, Problem 20.4(choose chapter or problem)
Assume that you want to construct a voltaic cell that uses the following half-reactions:
\(\mathrm{A}^{2+}(a q)+2 \mathrm{e}^{-} \longrightarrow \mathrm{A}(s) \quad E_{\text {red }}^{\circ}=-0.10 \mathrm{~V}\)
\(\mathrm{B}^{2+}(a q)+2 \mathrm{e}^{-} \longrightarrow \mathrm{B}(s) \quad E_{\mathrm{red}}^{\circ}=-1.10 \mathrm{~V}\)
You begin with the incomplete cell pictured here in which the electrodes are immersed in water.
(a) What additions must you make to the cell for it to generate a standard emf?
(b) Which electrode functions as the cathode?
(c) Which direction do electrons move through the external circuit?
(d) What voltage will the cell generate under standard conditions? [Sections 20.3 and 20.4]
Text Transcription:
{A}^{2+}(a q)+2 {e}^{-} \longrightarrow {A}(s) \quad E_red }}^{\circ}=-0.10 V
{B}^{2+}(a q)+2 {e}^{-} \longrightarrow {B}(s) \quad E_{red}}^{\circ}=-1.10 V
Unfortunately, we don't have that question answered yet. But you can get it answered in just 5 hours by Logging in or Becoming a subscriber.
Becoming a subscriber
Or look for another answer