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7. UJsing a curent of 4,75 A, how many minues toplae or10gaf Cfom a CuSO4 solution?...
9) A sol'n in an electrolytic cell contains the ions Cu2+, Fe2+ & Zn2+. If the voltage (initially...
9) A sol'n in an electrolytic cell contains the ions Cu2+, Fe2+ & Zn2+. If the voltage (initially very low) is turned up, in which order will the metals be plated out onto the cathode? Cu2+(aq)2e-Cu(s); E0.34V Fe"(aq) + 2e-→ Fe(s);E"--0.44V Zn2+(aq) + 2e-→ Zn(s): E。--0.76V 10) How long will it take to produce a sol'n of pH 2.00 by electrolysis of 500 mL of 0.100 M AgN03(aq) at 0.240 Amperes? Anode: 2H2O(l) → 4H-(aq) + O2(g) + 4e-, E°...
A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction: 2...
A voltaic cell operating under standard
conditions (1.0 M ion concentrations) utilizes the
following reaction:
2 Al(s) + 3 Ni2+(aq) 2 Al3+(aq) + 3 Ni(s)
What is the effect on the cell emf of each of the following
changes?
(a) Water is added to the cathode compartment, diluting the
solution.
The positive cell emf rises, becoming more positive.The positive
cell emf drops closer to zero. The
negative cell emf rises closer to zero.The negative cell emf drops,
becoming more negative.No change...
7. A is cell made by placing Zn(s) in Zn2 (aq) and Au(s) in Au (aq)....
7. A is cell made by placing Zn(s) in Zn2 (aq) and Au(s) in Au (aq). Use Standard Reduction Potentials. (12 points) a. Write the half reaction for the reaction at the cathode: Calculate the voltage for the standard cell (IM Zn2* (aq) and 1 M Au?* (aq). c. Calculate the voltage for the cell after it is 999% used up. Assume 1.00 L of each solution. (Hint: Write the overall equation.)
4. The following balanced redox reaction occurs in voltaic cell at 25°C H2 (g) + 2Ag+...
4. The following balanced redox reaction occurs in voltaic cell at 25°C H2 (g) + 2Ag+ (aq) → 2H* (aq) + 2 Ag (s) 2H+ + 2e → H2 (g) EⓇ = 0.00V Ag (aq) + le → Ag(s) E = +0.80V a. Write the two half-reactions (oxidation and reduction) occurring in the cell. Clearly indicate which reaction shows oxidation and which shows reduction. Clearly indicate which reaction occurs at the anode and which reaction occurs at the cathode. (4...
Please write out equation used, indicate the values used or ICE tables, when necessary. 7) Consider...
Please write out equation used, indicate the values used or ICE tables, when necessary. 7) Consider a galvanic cell based on the following two half reactions. Au3+ + 3 e Au? &_= +1.50 Agt + 1 e Ago & +0.80 Draw the appropriate battery, labeling cathode, anode, oxidation, reduction, direction of electron and ion flow. Calculate the voltage generated if [Ag+] = 0.25 M and [Au3+] = 1.25 M. Assume temperature is near standard conditions.
*redox reactions in electeochemical cells* c) Fe/0.1 M FeSO4//0.1 M CuSO4/Cu I soaked a porous cup in tap water for a few minutes and then i let it stand in a 100 ml beaker containing 10ml of 0.1 M Fe...
*redox reactions in electeochemical cells*
c) Fe/0.1 M FeSO4//0.1 M CuSO4/Cu
I soaked a porous cup in tap water for a few minutes and then i
let it stand in a 100 ml beaker containing 10ml of 0.1 M FeSO4. I
added enough 0.1M CuSO4 to the cup until the two liquid levels were
the same height. I inserted a zinc strip into the 0.1 M FeSO4 and a
shiny copper strip into the 0.1 M CuSO4. I connected the...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution of NaCl be used instead of NaNO3? 7. What was the purpose of FeSO4 solution in this experiment? 8. Could a solution of FeCl, be used instead of FeSO4? 9. Could a solution of NaSO4 be used instead of FeSO4? 10. Calculate the standard cell potential for the spontaneous redox reaction between a Pb(s)/Pb(NO3)2(aq) half-cell and a Ag(s)/AgNO3(aq) half-cell. Which metal would be oxidized?...
need help with the rest of the table EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE...
need help with the rest of the table
EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
Part 1.) Part 2.) A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes...
Part 1.)
Part 2.)
A voltaic cell operating under standard
conditions (1.0 M ion concentrations) utilizes the
following reaction:
2 Al(s) + 3 Ni2+(aq) 2
Al3+(aq) + 3 Ni(s)
What is the effect on the cell emf of each of the following
changes?
(a) Water is added to the cathode compartment, diluting the
solution:
The positive cell emf rises, becoming more positive. The positive
cell emf drops closer to zero. The negative cell emf rises closer
to zero. The negative...
please help answer question 4, a-f please using the data below from chart 1 objectives from...
please help answer question 4, a-f please
using the data below from chart 1
objectives from lab, thank you
DATA:CA y 3 Ay No3 Part I: Cell Potential of voltaic cells under standard conditions: cell CU CND2 #27 14.0m Give the half Half cell reaction at Combinations Oxidation Reduction E the anode and with [ion] takes place Theoretical takes place cathode. Write in M here here (V) above the arrow E c (V) if it is oxidation or reduction. |-0.340...
9) A sol'n in an electrolytic cell contains the ions Cu2+, Fe2+ & Zn2+. If the voltage (initially very low) is turned up, in which order will the metals be plated out onto the cathode? Cu2+(aq)2e-Cu(s); E0.34V Fe"(aq) + 2e-→ Fe(s);E"--0.44V Zn2+(aq) + 2e-→ Zn(s): E。--0.76V 10) How long will it take to produce a sol'n of pH 2.00 by electrolysis of 500 mL of 0.100 M AgN03(aq) at 0.240 Amperes? Anode: 2H2O(l) → 4H-(aq) + O2(g) + 4e-, E°...
A voltaic cell operating under standard
conditions (1.0 M ion concentrations) utilizes the
following reaction:
2 Al(s) + 3 Ni2+(aq) 2 Al3+(aq) + 3 Ni(s)
What is the effect on the cell emf of each of the following
changes?
(a) Water is added to the cathode compartment, diluting the
solution.
The positive cell emf rises, becoming more positive.The positive
cell emf drops closer to zero. The
negative cell emf rises closer to zero.The negative cell emf drops,
becoming more negative.No change...
7. A is cell made by placing Zn(s) in Zn2 (aq) and Au(s) in Au (aq). Use Standard Reduction Potentials. (12 points) a. Write the half reaction for the reaction at the cathode: Calculate the voltage for the standard cell (IM Zn2* (aq) and 1 M Au?* (aq). c. Calculate the voltage for the cell after it is 999% used up. Assume 1.00 L of each solution. (Hint: Write the overall equation.)
4. The following balanced redox reaction occurs in voltaic cell at 25°C H2 (g) + 2Ag+ (aq) → 2H* (aq) + 2 Ag (s) 2H+ + 2e → H2 (g) EⓇ = 0.00V Ag (aq) + le → Ag(s) E = +0.80V a. Write the two half-reactions (oxidation and reduction) occurring in the cell. Clearly indicate which reaction shows oxidation and which shows reduction. Clearly indicate which reaction occurs at the anode and which reaction occurs at the cathode. (4...
Please write out equation used, indicate the values used or ICE tables, when necessary. 7) Consider a galvanic cell based on the following two half reactions. Au3+ + 3 e Au? &_= +1.50 Agt + 1 e Ago & +0.80 Draw the appropriate battery, labeling cathode, anode, oxidation, reduction, direction of electron and ion flow. Calculate the voltage generated if [Ag+] = 0.25 M and [Au3+] = 1.25 M. Assume temperature is near standard conditions.
*redox reactions in electeochemical cells*
c) Fe/0.1 M FeSO4//0.1 M CuSO4/Cu
I soaked a porous cup in tap water for a few minutes and then i
let it stand in a 100 ml beaker containing 10ml of 0.1 M FeSO4. I
added enough 0.1M CuSO4 to the cup until the two liquid levels were
the same height. I inserted a zinc strip into the 0.1 M FeSO4 and a
shiny copper strip into the 0.1 M CuSO4. I connected the...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution of NaCl be used instead of NaNO3? 7. What was the purpose of FeSO4 solution in this experiment? 8. Could a solution of FeCl, be used instead of FeSO4? 9. Could a solution of NaSO4 be used instead of FeSO4? 10. Calculate the standard cell potential for the spontaneous redox reaction between a Pb(s)/Pb(NO3)2(aq) half-cell and a Ag(s)/AgNO3(aq) half-cell. Which metal would be oxidized?...
need help with the rest of the table
EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
Part 1.)
Part 2.)
A voltaic cell operating under standard
conditions (1.0 M ion concentrations) utilizes the
following reaction:
2 Al(s) + 3 Ni2+(aq) 2
Al3+(aq) + 3 Ni(s)
What is the effect on the cell emf of each of the following
changes?
(a) Water is added to the cathode compartment, diluting the
solution:
The positive cell emf rises, becoming more positive. The positive
cell emf drops closer to zero. The negative cell emf rises closer
to zero. The negative...
please help answer question 4, a-f please
using the data below from chart 1
objectives from lab, thank you
DATA:CA y 3 Ay No3 Part I: Cell Potential of voltaic cells under standard conditions: cell CU CND2 #27 14.0m Give the half Half cell reaction at Combinations Oxidation Reduction E the anode and with [ion] takes place Theoretical takes place cathode. Write in M here here (V) above the arrow E c (V) if it is oxidation or reduction. |-0.340...
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