The standard reduction potential of the process
The standard reduction potential of the process
$$ \mathrm{Zn}(\mathrm{OH})_{2}(\mathrm{~s})+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{Zn}(\mathrm{s})+2 \mathrm{OH}^{-}(\mathrm{aq}) $$
is \(E^{\circ}=-1.221 \mathrm{~V}\). Given that the standard reduction potential of the half-reaction
$$ \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(\mathrm{s}) $$
is \(E^{\circ}=-0.762 \mathrm{~V}\), find \(K_{\text {sp }}\) for \(Z \mathrm{n}(\mathrm{OH})_{2}\).
Kap = _______
Homework Answers
Given the following reaction determine (in kJ), and for the following reaction at...
23. (6pt) Given the following reaction determine \(\triangle G_{\text {ron }}^{\circ}(\) in \(K J)\), and \(K\) for the following reaction at \(25^{\circ} \mathrm{C}\) ? Is this reaction spontaneous?$$ 4 \mathrm{MnO}_{4}+12 \mathrm{H}^{*} \rightarrow 4 \mathrm{Mn}^{2+}+6 \mathrm{H}_{2} \mathrm{O}+5 \mathrm{O}_{2} $$\(\frac{\text { Reduction } 1 / 2 \text { Rxns }}{\mathrm{MnO}_{4}^{\circ}+8 \mathrm{H}^{*}+5 e^{\circ}} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) red: \(+1.49 \mathrm{~V}\)\(\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{*} \rightarrow \mathrm{2H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) rod \(+1.23 \mathrm{~V}\)
Question 23 The standard reduction potential of H,O2 = +1.763 V. Which of the following species...
Question 23 The standard reduction potential of H,O2 = +1.763 V. Which of the following species will be oxidized by hydrogen peroxide? End Co?"(aq) - Col(aq) +26 Ag(s) - Ag (aq) + € Co(s) - Co2+(aq) +26 Zn(s) -- Zr? (aq) + 2€ Na(s) Na (aq) + +1.953 V +0.799 V -0.282 V -0.762 V -2.714 V Ag(s), Co(s), Zn(s), and Na(s) Co- and Ag(s) Co(s) and Co2+ Zn(s) and Na(s) Code
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Cl...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Cl 2 (g) + 2 e − → 2 Cl − (aq) = E 0 red + 1.359 V MnO − 4 (aq) + 2 H 2 O (l) + 3 e − → MnO 2 (s) + 4 OH − (aq) = E 0 red + 0.59 V cathode half reaction anode half reaction overall reaction cell potential at standard state
Lithium ion batteries use the two half-reactions whose standard reduction potentials are shown below. CoO_2 (s)...
Lithium ion batteries use the two half-reactions whose standard reduction potentials are shown below. CoO_2 (s) + Li^+ (aq) + e^- rightarrow LiCoO_2 E degree = 1.0 V Li^+ (aq) + C_6 (s) + e^- rightarrow LiC_6 E degree = -3.0 V Write the balance overall equation for the spontaneous oxidation-reduction reaction that occurs in lithium ion batteries, Calculate the standard potential and standard free energy change for the process.
Suppose there were a new scale for expressing electrode potentials in which the standard potential for...
Suppose there were a new scale for expressing electrode potentials in which the standard potential for the reduction of water in base: 2 H_2O(l) + 2 e^- rightarrow H_2 (g) + 2 OH^- (aq) is assigned an E degree_red value of 0.000 V. In current standard reduction tables, the following reaction has a standard reduction potential of 1.50 V. M^3+ (aq) + 3 e^- rightarrow M(s) What would the reduction potential be on the new scale in which the reduction...
What is the standard potential for the redox titration in this lab if the standard reduction...
What is the standard potential for the redox titration in this lab if the standard reduction potential at 25 degree for oxalate (below) is -0.430 V? What is Delta G degree for the redox reaction? Why then does the reaction need to be heated? 2 CO_2(g) + 2 H_3O^+(aq) + 2e^- rightarrow H_2C_2O_4(aq) E degree = -0.430 V
Calculate E°cell for the following reaction:?? 2Fe2+(aq) + Cd2+(aq) ? 2Fe3+(aq) + Cd(s)
Calculate \(E_{\text {cell }}^{\circ}\) for a iron-cadmium cell in which the cell reaction is$$ 2 \mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{Cd}^{2+}(\mathrm{aq}) \rightarrow 2 \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{Cd}(\mathrm{s}) $$$$ \begin{array}{ll} \mathrm{Fe}^{3+}+e^{-} \rightarrow \mathrm{Fe}^{2+} & E^{\mathrm{O}}=0.77 \mathrm{~V} \\ \mathrm{Cd}^{2+}+2 e^{-} \rightarrow \mathrm{Cd} & E^{\mathrm{O}}=-0.40 \mathrm{~V} \end{array} $$is oxidized in the reaction: \(2 \mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{Cd}^{2+}(\mathrm{aq}) \rightarrow 2 \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{Cd}(\mathrm{s})\)Select one:A. -0.37 VB. 0.37 VC. -1.17 VD. 1.17 VE. none of these
The standard reduction potential of the Pb2+|Pb electrode is –0.13 V and the standard potential of...
The standard reduction potential of the Pb2+|Pb electrode is –0.13 V and the standard potential of the cell Zn(s) | Zn2+(aq) || Pb2+(aq) | Pb(s) is +0.63 V. What is the standard reduction potential of the Zn2+|Zn electrode? Question 9 options: –0.76 V –1.52 V +0.76 V –0.50 V +0.50 V
half-reaction standard reduction potential Zn?" (aq)+2e" - Zn(s) Epod= -0.763 V MnO, (aq)+2 H,0(1+3e" - MnO,(s)+4...
half-reaction standard reduction potential Zn?" (aq)+2e" - Zn(s) Epod= -0.763 V MnO, (aq)+2 H,0(1+3e" - MnO,(s)+4 OH (aq). E = +0.59 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. X 5 ? Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written Yes Do you have...
Calculate the cell potential difference, Eºcell (Ecell = Eºcathode - Eanode), given the standard reduction potential...
Calculate the cell potential difference, Eºcell (Ecell = Eºcathode - Eanode), given the standard reduction potential below, Cut2 (aq) + 2 e. ----> Cu (s) ° = 0.337 volts Pb+2 (aq) + 2 e--...-> Pb(s) ° = -0.126 volts 0.211 V 0.463 V -0.463 V -0.211 V In Part III, to light up a white LED bulb will require forward voltage (VF) at 20 mA. • 5 1.2. 2.0 Calculate the cell potential difference, Eºcell ( cell = Eºcathode -...
23. (6pt) Given the following reaction determine \(\triangle G_{\text {ron }}^{\circ}(\) in \(K J)\), and \(K\) for the following reaction at \(25^{\circ} \mathrm{C}\) ? Is this reaction spontaneous?$$ 4 \mathrm{MnO}_{4}+12 \mathrm{H}^{*} \rightarrow 4 \mathrm{Mn}^{2+}+6 \mathrm{H}_{2} \mathrm{O}+5 \mathrm{O}_{2} $$\(\frac{\text { Reduction } 1 / 2 \text { Rxns }}{\mathrm{MnO}_{4}^{\circ}+8 \mathrm{H}^{*}+5 e^{\circ}} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) red: \(+1.49 \mathrm{~V}\)\(\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{*} \rightarrow \mathrm{2H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) rod \(+1.23 \mathrm{~V}\)
Question 23 The standard reduction potential of H,O2 = +1.763 V. Which of the following species will be oxidized by hydrogen peroxide? End Co?"(aq) - Col(aq) +26 Ag(s) - Ag (aq) + € Co(s) - Co2+(aq) +26 Zn(s) -- Zr? (aq) + 2€ Na(s) Na (aq) + +1.953 V +0.799 V -0.282 V -0.762 V -2.714 V Ag(s), Co(s), Zn(s), and Na(s) Co- and Ag(s) Co(s) and Co2+ Zn(s) and Na(s) Code
Lithium ion batteries use the two half-reactions whose standard reduction potentials are shown below. CoO_2 (s) + Li^+ (aq) + e^- rightarrow LiCoO_2 E degree = 1.0 V Li^+ (aq) + C_6 (s) + e^- rightarrow LiC_6 E degree = -3.0 V Write the balance overall equation for the spontaneous oxidation-reduction reaction that occurs in lithium ion batteries, Calculate the standard potential and standard free energy change for the process.
Suppose there were a new scale for expressing electrode potentials in which the standard potential for the reduction of water in base: 2 H_2O(l) + 2 e^- rightarrow H_2 (g) + 2 OH^- (aq) is assigned an E degree_red value of 0.000 V. In current standard reduction tables, the following reaction has a standard reduction potential of 1.50 V. M^3+ (aq) + 3 e^- rightarrow M(s) What would the reduction potential be on the new scale in which the reduction...
What is the standard potential for the redox titration in this lab if the standard reduction potential at 25 degree for oxalate (below) is -0.430 V? What is Delta G degree for the redox reaction? Why then does the reaction need to be heated? 2 CO_2(g) + 2 H_3O^+(aq) + 2e^- rightarrow H_2C_2O_4(aq) E degree = -0.430 V
half-reaction standard reduction potential Zn?" (aq)+2e" - Zn(s) Epod= -0.763 V MnO, (aq)+2 H,0(1+3e" - MnO,(s)+4 OH (aq). E = +0.59 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. X 5 ? Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written Yes Do you have...
Calculate the cell potential difference, Eºcell (Ecell = Eºcathode - Eanode), given the standard reduction potential below, Cut2 (aq) + 2 e. ----> Cu (s) ° = 0.337 volts Pb+2 (aq) + 2 e--...-> Pb(s) ° = -0.126 volts 0.211 V 0.463 V -0.463 V -0.211 V In Part III, to light up a white LED bulb will require forward voltage (VF) at 20 mA. • 5 1.2. 2.0 Calculate the cell potential difference, Eºcell ( cell = Eºcathode -...
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