How many grams of zinc, Zn (s) are electroplated out of a solution containing Zn2+ (aq)...

How many grams of zinc, Zn (s) are electroplated out of a solution containing Zn2+ (aq) if the solution is electrolyzed for 1 hour 22 minutes and 26 seconds at current of 1.22 amps?

In an experiment similar to this one, a polished strip of Cu (s) was found to weigh 17.452 g. This strip was electrolyzed for exactly 25 minutes at an average current of 0.987 amps. The weight of the copper strip after electrolysis was 17.996 g. From these data, calculate the value of the Faraday constant.

Expert Solution

queen_honey_blossom answered 2 years ago

The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2 (aq, 0.100 M)||Zn2 (aq, ?...

The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2 (aq, 0.100 M)||Zn2 (aq, ? M)|Zn(s) is 26.0 mV at 25 °C. Calculate the concentration of the Zn2 (aq) ion at the cathode.

complete and balance the net ionic equations for reactions that would occur: Zn(s)+Mg2+(aq)---> Zn(s)+Cu2+(aq)----> Zn(s)+H+(aq)-----> Mg(s)+Zn2+(aq)----->...

complete and balance the net ionic equations for reactions that would occur: Zn(s)+Mg2+(aq)---> Zn(s)+Cu2+(aq)----> Zn(s)+H+(aq)-----> Mg(s)+Zn2+(aq)-----> Mg(s)+Cu2+(aq)---> Mg(s)+H+(aq)----> Cu(s)+Zn2+(aq)----> Cu(s)+Mg2+(aq)----> Cu(s)+H+(aq)----->

ZnCl2 (aq) + Al (s) ---- Zn(s) + AlCl3 (aq) [Al3+] = 0.8 M [Zn2+] =...

ZnCl2 (aq) + Al (s) ---- Zn(s) + AlCl3 (aq) [Al3+] = 0.8 M [Zn2+] = 1.3M Zn2+(aq) +2e- ---Zn(s) -0.76V Al3+(aq) + 3e- --- Al (s) -1.66V Balance the equation above. Give the equation for the reaction quotient(Q) and solve for it. Are there units for (Q)? Solve for the standard potential for the cell (EO cell) at 295K. First give equation. Solve the Nernst equation for this cell at 295K.

The standard cell potential, E°, for Br2(aq) + Zn(s) → 2Br-(aq) + Zn2+(aq) at 298K is...

The standard cell potential, E°, for Br2(aq) + Zn(s) → 2Br-(aq) + Zn2+(aq) at 298K is 1.82V. Calculate the value of ΔG° in kJ. Use 96,485 C/mol e-. Then calculate the equilibrium constant for the data.

calculate the Electromotive Force (E) at 298 K for Zn(s) + Sn4+(aq) <-> Zn2+(aq) + Sn2+(aq)...

calculate the Electromotive Force (E) at 298 K for Zn(s) + Sn4+(aq) <-> Zn2+(aq) + Sn2+(aq) If [Sn4+] = 0.21 [Zn2+] = 0.44 [Sn2+] = 0.21 Assume that γ±γ± = 0.82 for all species. Give your answer in volts to three decimal places (X.XXX).

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) How many...

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) How many liters of H2 would be formed at 636 mm Hg and 17 ∘C if 27.0 g of zinc was allowed to react? How many grams of zinc would you start with if you wanted to prepare 6.85 L of H2 at 284 mm Hg and 28.5 ∘C?

Given the following reaction, Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq) E° = 1.10 V. Use...

Given the following reaction, Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq) E° = 1.10 V. Use the Nernst equation to calculate the cell potential for the cell described with standard line notation below. Zn|Zn2+(0.5082 M)||Cu2+(0.2699 M)|Cu Units are not required. Report answer to three decimal places. Please explain all of your steps! Thanks!

3) Consider a voltaic cell in which the following reaction occurs: Zn(s) + Sn2+(aq)  Zn2+(aq)...

3) Consider a voltaic cell in which the following reaction occurs: Zn(s) + Sn2+(aq)  Zn2+(aq) + Sn(s) a) Calculate Eo for the cell. b) when the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+ ? c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+ ? d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the...

Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚...

Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚ for the reaction, given that: ∆Gf Zn(s) = 0, ∆Gf(H+) = 0, ∆Gf(H2) = 0, ∆Gf(Zn2+) = -147.1 kj/mol b) ∆G, when P(h2) = 750 mmHg, [Zn2+ aq] = 0.10 M, [H+] = 1.0 x 10^-4 M c) The pH when ∆G - -100 kJ, P(h2) = 0.922 atm, [Zn2+] = 0.200 M and the mass of Zn is 155 g.

Consider the Daniell cell, for which the overall cell reaction is Zn(s)+Cu2+(aq)⇌Zn2+(aq)+Cu(s) The concentrations of CuSO4...

Consider the Daniell cell, for which the overall cell reaction is Zn(s)+Cu2+(aq)⇌Zn2+(aq)+Cu(s) The concentrations of CuSO4 and ZnSO4 are 2.20×10−3 m and 1.10×10−3 m , respectively. A) Calculate E setting the activities of the ionic species equal to their molalities. Express your answer to four significant figures and include the appropriate units. B) Calculate γ±,ZnSO4 for the half-cell solutions using the Debye-Huckel limiting law. Express your answer using three significant figures. C) Calculate γ±,CuSO4 for the half-cell solutions using the...

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