A voltaic cell is constructed from a standard Cd2+ | Cd half cell (EĀ°red = -0.403V) and a standard Fe3+ | Fe2+ half cell (EĀ°red = 0.771V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is V.
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A voltaic cell is constructed from a standard Ag+ | Ag half-cell (EĆĀ° red = 0.799 V) and a standard Cr3+ | Cr half-cell (EĆĀ° red = -0.740 V). The anode reaction is: Ag(s) -> Ag+(aq) + e- The cathode reaction is: Cr3+(aq) + 3e- -> Cr(s) The spontaneous cell reaction is: Ag(s) + Cr3+(aq) -> Ag+(aq) + Cr(s) The cell voltage is _______ V.
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A voltaic cell that uses the reaction $$ \operatorname{PdCl}_{4}^{2-}(a q)+\mathrm{Cd}(s) \longrightarrow \mathrm{Pd}(s)+4 \mathrm{Cl}^{-}(a q)+\mathrm{Cd}^{2+}(a q) $$ has a measured standard cell potential of $+1.03 \mathrm{V}$ . (a) Write the two half-cell reactions. (b) By using data from Appendix E, determine $E_{\text { red }}^{\circ}$ for the reaction involving Pd. (c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow.
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