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ourses / chem12_51_16b / UNIT 5: ELECTROCHE Given the following electrochemical cell, label apropriately and answer...
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge....
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. a Fe electrode in 1.0 M FeCl2 solution a Sn electrode in 1.0 M Sn(NO3)2 solution Fe2+ + 2e- → Fe Eo = -0.44 V Sn2+ + 2e- → Sn Eo = -0.14 V When the cell is running spontaneously, which choice includes only true statements and no false ones? Select one: a. The iron electrode gains mass and the iron electrode is the...
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + €...
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + € → Fe2+ +0.77 v +0.34 V -0.13 V Cu2+ +2e → Cu Pb2+ + 2e - → Ib Ni2+ + 2e → Ni Cd2+ +2e → Cd -0.25 V -0.40 V Fe2+ + 2e → Fe -0.44 V Zn2+ + 2e → Zn -0.76 V Al3+ +3e → AI - 1.66 V Consider an electrochemical cell constructed from the following half cells, linked by...
Questions 1. Answer the following questions about this electrochemical cell: NiNi(0.100M)||Fe (0.050M), Fe (0.050M)P a. Give...
Questions 1. Answer the following questions about this electrochemical cell: NiNi(0.100M)||Fe (0.050M), Fe (0.050M)P a. Give the balanced chemical equation for the cell b. Calculate the cell potential c. Why is platinum used as the electrode on the cathode side? 2. What steps might you take to solve each of the following common problems when building an electrochemical cell: a. The digital multimeter reads "0" no matter what the setting on the dial. b. The reading "flickers on and off"...
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)...
6. Consider an electrochemical cell constructed from the following half cells, linked by an external cir-...
6. Consider an electrochemical cell constructed from the following half cells, linked by an external cir- cuit and by a KCl salt bridge. • an Als) electrode in 1.0 MAINO:)solution . a Pb(s) electrode in 1.0 MPb(NO3), solution 1. Which is oxidized? A. AI B. A C. Pь D. Pb? 2. Which is the half reaction at the anode? A. B. C. D. Pb() Pb(aa) +2e A1) Al (aq) +3e. Pb(aq) + 2e →Pb() Al (aa) +3e + Al(s) 3....
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
PLEASE ANSWER ALL 4. The cell potential for the unbalanced chemical reaction: Hg2 2+(aq) + NO3...
PLEASE ANSWER ALL 4. The cell potential for the unbalanced chemical reaction: Hg2 2+(aq) + NO3 - (aq) + H+ (aq) → Hg2+(aq) + HNO2(aq) is measured under standard conditions and found to be + 0.02 V at 25C. a) What substance (not just the element) is oxidized in the cell? b) What substance (not just the element) is reduced in the cell? c) Write the half-reaction that occurs in the anode compartment. d) Write the half-reaction that occurs in...
Table provided below for context Please answer all parts that you can. 1. Which electrochemical cell...
Table provided below for context
Please answer all parts that you can.
1. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 2. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 3. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is...
3. Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Answer: read 21.2, see sample...
3. Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Answer: read 21.2, see sample problem 21.2 A. Which metal is being oxidized? B. Which metal is being reduced? C. Identify and label the anode/cathode/salt bridge D. Salt bridge is made with potassium nitrate, show ion flow E. Which electrode decreases in mass during cell operation? F. In which direction do electrons flow in the external circuit? G. At which electrode are electrons generated?
Answer the following questions related to the givenelectrochemical cell under standard conditions.W3+(aq) + 3e−...
Answer the following questions related to the given electrochemical cell under standard conditions.W3+(aq) + 3e− ⇌ W(s)E° = 0.100 VCo2+(aq) + 2e− ⇌ Co(s)E° = -0.280 V1. Answer the following questions.(a) The half cell containing W/W3+ is the anode/ cathode(b) Which one of the following statements isTRUE for the half cell containing W and W3+.W3+ will be oxidized to form W.W3+ will be reduced to form W.W will be reduced to form W3+.W will be oxidized to form W3+.(c) The half...
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + € → Fe2+ +0.77 v +0.34 V -0.13 V Cu2+ +2e → Cu Pb2+ + 2e - → Ib Ni2+ + 2e → Ni Cd2+ +2e → Cd -0.25 V -0.40 V Fe2+ + 2e → Fe -0.44 V Zn2+ + 2e → Zn -0.76 V Al3+ +3e → AI - 1.66 V Consider an electrochemical cell constructed from the following half cells, linked by...
Questions 1. Answer the following questions about this electrochemical cell: NiNi(0.100M)||Fe (0.050M), Fe (0.050M)P a. Give the balanced chemical equation for the cell b. Calculate the cell potential c. Why is platinum used as the electrode on the cathode side? 2. What steps might you take to solve each of the following common problems when building an electrochemical cell: a. The digital multimeter reads "0" no matter what the setting on the dial. b. The reading "flickers on and off"...
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)...
6. Consider an electrochemical cell constructed from the following half cells, linked by an external cir- cuit and by a KCl salt bridge. • an Als) electrode in 1.0 MAINO:)solution . a Pb(s) electrode in 1.0 MPb(NO3), solution 1. Which is oxidized? A. AI B. A C. Pь D. Pb? 2. Which is the half reaction at the anode? A. B. C. D. Pb() Pb(aa) +2e A1) Al (aq) +3e. Pb(aq) + 2e →Pb() Al (aa) +3e + Al(s) 3....
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
Table provided below for context
Please answer all parts that you can.
1. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 2. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 3. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is...
3. Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Answer: read 21.2, see sample problem 21.2 A. Which metal is being oxidized? B. Which metal is being reduced? C. Identify and label the anode/cathode/salt bridge D. Salt bridge is made with potassium nitrate, show ion flow E. Which electrode decreases in mass during cell operation? F. In which direction do electrons flow in the external circuit? G. At which electrode are electrons generated?
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