What is the cell potential when the concentration of Ni has tallen to 0.600 mol L-2Express your answer to two decimal places and Include the appropriate units.A voltaic cell consists of a Zn/Zn+ halt-cell and aNi/NI+ half-cell at 25 C. The initialconcentrations of Ni* and Zn* are 1.70mol L- and O.130 mol L, rospectively.Ecel 0.52 VSubnitPrevious AnswersZn* (ag) +2 e + Zn(s)Ni (ag) +2 e - NI(s)E-0.76 VE =-0.23 Vv CorrectPart CWhat are the concentrations of Ni and Zn when the cell potential falls to 0.46 V?Express your answers using two significant figures separated by a comma.mol L-1SubmitBequest Answet

Given: Initial concentration of Ni+2 = 1.70 M Initial concentration of Zn+2 =0.130 M…

What is the cell potential when the concentration of Ni has fallen to 0.600 mol L Express your answer to two decimal places and Include the appropriate units A voltaic cell consists of a Zn/Zn hall-cell and a Ni/N* hall-ceoll at 25 "C. The initial concentrations of Ni and Zn are 1.70 mol L and 0.130 mol L, rospectively Eeeli 0.52 V Subnit Previous Answers Zn" (ag) +2 e Zn(a) E -0.76 V Ni" (ag) +2 e"- NI() E-0.23 V v Correct Part C What are the concentrations of NP and Zn when the cell potential falls to 0.46 V? Express your answers using two significant figures separated by a comma. ?. mol L Submit Bequest Answet

What is the cell potential when the concentration of Ni has fallen to 0.600 mol L Express your answer to two decimal places and Include the appropriate units A voltaic cell consists of a Zn/Zn hall-cell and a Ni/N* hall-ceoll at 25 "C. The initial concentrations of Ni and Zn are 1.70 mol L and 0.130 mol L, rospectively Eeeli 0.52 V Subnit Previous Answers Zn" (ag) +2 e Zn(a) E -0.76 V Ni" (ag) +2 e"- NI() E-0.23 V v Correct Part C What are the concentrations of NP and Zn when the cell potential falls to 0.46 V? Express your answers using two significant figures separated by a comma. ?. mol L Submit Bequest Answet

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter32: Voltaic Cell Measurements

Section: Chapter Questions

Problem 2ASA

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Similar questions

a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
Calculate the standard cell potential of the following cell at 25C. Sn(s)Sn2+(aq)I2(aq)I(aq)
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-.
At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)