Zn(s)+ MnO4-(aq)-> Zn2+(aq) +Mn2+(aq) write cell notation, equilibrium constant annd will this function as a battery?
Homework Answers
Pure solids and liquids are not included in the equilibrium constant expression. This is because they do not affect the reactant amount at equilibrium in the reaction, so they are disregarded and kept at 1. Remember that the activity, a, of any solid or liquid in a reaction is equal to 1
C) this reaction comes under redox reaction thus it can be
function as battery ![Given chemical reaction to Zu cgst Muoat cag] > Zut +Mit (aq) caq cell notation. Electrode material Ispecies rodie species ma](http://img.homeworklib.com/questions/1fcafb50-e99f-11ea-b944-6f2c992212cf.png?x-oss-process=image/resize,w_560)
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Zn(s)+ MnO4-(aq)-> Zn2+(aq) +Mn2+(aq)
write cell notation, equilibrium constant annd will this
function as a battery?
Given the following line notation for an electrochemical cell, write the balanced net equation: Zn(s) |...
Given the following line notation for an electrochemical cell, write the balanced net equation: Zn(s) | Zn2+ (aq, 1 M) || H+ (aq, 1 M), MnO4 - (1 M), Mn2+ (1 M) | Pt
Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+ (aq) and a...
Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+ (aq) and a cathode where Co+ (aq) is reduced to Co (s). Assume all aqueous solutions have a concentration of 1 moVL
Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+ (aq) and a cathode where Co+ (aq) is reduced to Co (s). Assume all aqueous solutions have a concentration of...
The voltage generated by the zinc concentration cell described by the line notation Zn(s) || Zn2+(aq,0.100...
The voltage generated by the zinc concentration cell described by the line notation Zn(s) || Zn2+(aq,0.100 M) ‖‖ Zn2+(aq,? M) || Zn(s)Zn(s) | Zn2+(aq,0.100 M) ‖ Zn2+(aq,? M) | Zn(s) is 16.0 mV16.0 mV at 25 °C.25 °C. Calculate the concentration of the Zn2+(aq)Zn2+(aq) ion at the cathode.
Consider the cell represented by the following line notation: Zn(s) | Zn2+ (aq) || ClO2 (aq)|...
Consider the cell represented by the following line notation: Zn(s) | Zn2+ (aq) || ClO2 (aq)| ClO2(g) | Pt(s) Assuming standard conditions, calculate Eºcell: Zn2+ (aq) + 2e - Zn(s) E' = -0.76 V ClO2(g) + e - ClO2 (aq) F° = 0.95 V Express your answer to two decimal places. Eºcell
The voltage generated by the zinc concentration cell described by the line notation Zn(s) | Zn2+(aq,0.100...
The voltage generated by the zinc concentration cell described by the line notation Zn(s) | Zn2+(aq,0.100 M) || Zn2+(aq, ? M)| Zn(s) is 12.0 mV at 25 °C. Calculate the concentration of the Zn2+ (aq) ion at the cathode. concentration: concentration:
The half-cell reactions that occur in a typical flashlight battery are: Zn(s) -7 Zn²+ (aq) +...
The half-cell reactions that occur in a typical flashlight battery are: Zn(s) -7 Zn²+ (aq) + 2 e 2 MnOz(s) + Zn2+ (aq) + 2 e -7 ZnMn20_(5) Write a chemical equation describing the net cell reaction
Balance the following redox reaction in acidic solution.... Mn2+(aq)+Zn2+(aq)=MnO2(s)+Zn(s)
Balance the following redox reaction in acidic solution.... Mn2+(aq)+Zn2+(aq)=MnO2(s)+Zn(s)
Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is...
Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+(aq) and a cathode where Ni2+(aq) is reduced to Ni (s) . Assume all aqueous solutions have a concentration of 1 mol/L.
A) Write the cell notation for an electrochemical cell consisting of an anode where Mn (s)...
A) Write the cell notation for an electrochemical cell consisting of an anode where Mn (s) is oxidized to Mn2+(aq) and a cathode where Cd2+(aq) is reduced to Cd (s) . Assume all aqueous solutions have a concentration of 1 mol/L. B) Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+(aq) and a cathode where H+(aq) is reduced to H2(g) at a platinum electrode . Assume all aqueous solutions have...
answer plz Question 32 (3 points) (32) For a galvanic cell notation: (-) Zn /Zn2+ (aq)...
answer plz
Question 32 (3 points) (32) For a galvanic cell notation: (-) Zn /Zn2+ (aq) // Cu2+ (aq) / Cu (+), which of the following is fully correct? (a) Zn2+ is oxidized to Zn, and Cu2+ (aq) is reduced to Cu. (b) Zn is oxidized to Zn2+, and Cu2+ (aq) is reduced to Cu. 0 (c) Zn2+ is reduced to Zn, and Cu2+ (aq) is oxidized to Cu. (d) Zn is reduced to Zn2+, and Cu (aq) is reduced...
Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+ (aq) and a cathode where Co+ (aq) is reduced to Co (s). Assume all aqueous solutions have a concentration of 1 moVL
Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+ (aq) and a cathode where Co+ (aq) is reduced to Co (s). Assume all aqueous solutions have a concentration of...
Consider the cell represented by the following line notation: Zn(s) | Zn2+ (aq) || ClO2 (aq)| ClO2(g) | Pt(s) Assuming standard conditions, calculate Eºcell: Zn2+ (aq) + 2e - Zn(s) E' = -0.76 V ClO2(g) + e - ClO2 (aq) F° = 0.95 V Express your answer to two decimal places. Eºcell
The voltage generated by the zinc concentration cell described by the line notation Zn(s) | Zn2+(aq,0.100 M) || Zn2+(aq, ? M)| Zn(s) is 12.0 mV at 25 °C. Calculate the concentration of the Zn2+ (aq) ion at the cathode. concentration: concentration:
The half-cell reactions that occur in a typical flashlight battery are: Zn(s) -7 Zn²+ (aq) + 2 e 2 MnOz(s) + Zn2+ (aq) + 2 e -7 ZnMn20_(5) Write a chemical equation describing the net cell reaction
answer plz
Question 32 (3 points) (32) For a galvanic cell notation: (-) Zn /Zn2+ (aq) // Cu2+ (aq) / Cu (+), which of the following is fully correct? (a) Zn2+ is oxidized to Zn, and Cu2+ (aq) is reduced to Cu. (b) Zn is oxidized to Zn2+, and Cu2+ (aq) is reduced to Cu. 0 (c) Zn2+ is reduced to Zn, and Cu2+ (aq) is oxidized to Cu. (d) Zn is reduced to Zn2+, and Cu (aq) is reduced...
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