Answer my question please - The following graph representsthe Relation between time andmass ofPrecipitate copper when passingElectricity in CuSO4 solution usinginert Electrodes.Mass of copper (g)0.500.400.300.200.10T(sec)10203040Study the graph well then answer:- The anode half reaction is(a) 2H*(aq) + 2e → H2 (g)(b) 4H*(aq)+ 4e → H2 (g)(C) 2Cu**(aq)+ 4e → 2Cu (s)(d) Cu+(aq)+ 2e → Cu (s)abCII - The anode half reaction is(а) 20H:→ 2H+(aq) + 02 (g) + 4e(аq)(b) 40Н (ag)→ 4H*(aq)+ 202 (g)+ 8e(C) so-4(aq)→ SO2 (ag) + O2 (g) + 2e(d) 2S0 4(aq)→ 2S02 (ag) + 02 (g) +4eabd- The electric current intensitypassed in the electrolyteequal.(а) 20A(b) 40A(C) 50A(d) 60AII

The chemical decomposition brought about by the passage of electricity through an electrolyte in the…

- The following graph represents the Relation between time and mass of Precipitate copper when passing Electricity in Cuso4 solution using inert Electrodes. Mass of copper (8) 0.50 0.40 0.30 0.20 0.10 T(sec) 10 20 30 40 Study the graph well then answer: - The anode half reaction is ....... (а) 2H* + 2e → H2 (g) (aq) (b) 4H* (aq) + 4e → H2 (g) (C) 2Cu++ (aq) + 4e → 2Cu (s) (d) Cu*+ (ag) + 2e → Cu (s) a b

- The following graph represents the Relation between time and mass of Precipitate copper when passing Electricity in Cuso4 solution using inert Electrodes. Mass of copper (8) 0.50 0.40 0.30 0.20 0.10 T(sec) 10 20 30 40 Study the graph well then answer: - The anode half reaction is ....... (а) 2H* + 2e → H2 (g) (aq) (b) 4H* (aq) + 4e → H2 (g) (C) 2Cu++ (aq) + 4e → 2Cu (s) (d) Cu*+ (ag) + 2e → Cu (s) a b

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 105E: A solution at 25C contains 1.0 M Cd2+, 1.0 M Ag+, 1.0 M Au3+, and 1.0 M NiH2+ in the cathode...

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Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
What is the voltage of a concentration cell of Cl ions where the concentrations are 1.045 and 0.085 M? What the spontaneous reaction?
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° 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 voltage drops to zero?
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
A solution at 25C contains 1.0 M Cd2+, 1.0 M Ag+, 1.0 M Au3+, and 1.0 M NiH2+ in the cathode compartment of an electrolytic cell. Predict the order in which the metals will plate out as the voltage is gradually increased.
Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as shown: Ag+(aq)+NH3(aq)AgNH3+(aq)K1=2.1103AgNH3+(aq)+NH3(aq)Ag(NH3)2+(aq)K2=8.2103 Calculate the cell potential after the addition of 15.0 moles of NH3.