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Part B: Cell Potential and Temperature (Pb/Cu cell) 1. Fill in the table. Use cell one...
Effect of Temperature on Cell Potential Cell designation: E (measured) Temperature (°C) PbPb2+ || Cu2+ Cu;...
Effect of Temperature on Cell Potential Cell designation: E (measured) Temperature (°C) PbPb2+ || Cu2+ Cu; 0.455 Temperature (K) AG (calculated) 0.497 295 0.512 Sn Sn2+ || Cult | Cu; 0.548 0.554 279 295 0.566 343 Y AS determined from the slope of a plot of AG versus T AS Pb Cur AS Sn|Cu = AH° Pb | Cu=- AHSn Cu=- AHº calculated at 298 K (show calculations) from AG = AH-TAS AH = AG+TAS
Electrochemical Cells and Thermodynamics Key (calculated) Shorthand cell designation ΔΟ (calculated) E cell (measured) Temperature ( ) and Keq for an exemplary pair. For Pb | Pb2+ Isn2+ Sn: Show c...
Electrochemical Cells and Thermodynamics Key (calculated) Shorthand cell designation ΔΟ (calculated) E cell (measured) Temperature ( ) and Keq for an exemplary pair. For Pb | Pb2+ Isn2+ Sn: Show calculations for E half-cell (calculated) Half-cell equation Effect of Temperature on Cell Potential Cell designation: E (measured Tempegature fc) Temperature (kK) AG (calculated) 5 c 1134 228 K 2315 AS determined from the slope of a plot of AG versus T (show calculations) AfP calculated at 298 K 233
Electrochemical...
Ive attacthed all my results. I just need help calculating question 4 and 5 (5 pts)...
Ive
attacthed all my results. I just need help calculating question 4
and 5
(5 pts) Part II. Your experimental data: how many sig figs should your temperature data have? Show work for one calculation of temp in Kelvin. Show work for one AG calculation: Approximate Measured Cell Calculated Temp (°C) Calculated Temp (°C) potential Temp (K) AG Ecell (V)* (kJ/mol)* * measured value 70.21 0.581 343 1-112.1 65.12 0.680338 - 111.9 Show work: 60.02 0.5715333 -1110 °C -> 5.05+278.15...
equation in graph: E=1.13E+00-1.08E-04T 8. (10 pts) A cell is constructed Cu2+ to Cu, while the zinc is oxidized from Zn to Zn+. The cell potential is measured as temperature, yielding the graph...
equation in graph: E=1.13E+00-1.08E-04T
8. (10 pts) A cell is constructed Cu2+ to Cu, while the zinc is oxidized from Zn to Zn+. The cell potential is measured as temperature, yielding the graph below. with a copper anode and a zinc cathode. The copper is reduced from 1 3E-00-1.08E-04 T e» 1 8 280 290 300 310 320 330 340 350 Determine Δrrn // and ΔrrnS for this reaction from the data given.
8. (10 pts) A cell is constructed...
Data Sheet Part A: Dependence of Reaction Rate on Concentration Table 1 H Temperature Time Relati...
Can someone please help me finish the tables and
calculations.
Thanks in advance
Data Sheet Part A: Dependence of Reaction Rate on Concentration Table 1 H Temperature Time Relative mixture ! (seconds) | rate 1000 Reaction BrOsl (eC) . 1235.6 Avg. time 2. 67.S 3. 08,24 Avg. time 2. 74.2 3. 70.74.O Avg. time 24.o' 4 弘·11 0.2 OD3 0.00 8 100 o.oy | 23.5 3. 29. Avg. time 교 Table 2: Calculations for the [I']. [Bro, & [H'] BrOs...
use tabulated standard electrode potential to calculate the standard cell potential for the reaction occurring in an el...
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
Partner's Name Instructor Procedure I, Voltaic Cell Zn/Zn2+ 1.0 M || Cu2+ 1.0 M/Cu In the...
Partner's Name Instructor Procedure I, Voltaic Cell Zn/Zn2+ 1.0 M || Cu2+ 1.0 M/Cu In the space below write the equations for the two half reactions and sum them appropriately to calculate the standard reaction potential for a 1.0 M voltaic cell. Show the overall net ionic equation for this reaction. 9pts.) Standard reaction potential Write the expression for Q for this redox reaction. (4 pes) In the space below show a calculation using the Nemst equation to determine the...
how do I solve this? 1. Use the Nernst equation to calculate the standard cell potential...
how
do I solve this?
1. Use the Nernst equation to calculate the standard cell potential for a voltaic cell of a Sn electrode in 0.10M Sn2(a) in one half-cell and Al in 0.10M AP) in the other. (EPe Eaode- Emode 1.52 V, Show your work. Hint: Check E values of the reduction haif reactions. Write the one with more negative E as oxidation half reaction (change the sign); ensure that equal number of electrons are exchanged ie. electrons cancel,...
Cell Potential and Equilibrium Standard reduction potentials The equilibrium constant, K, for a redox reaction is...
Cell Potential and Equilibrium Standard reduction potentials The equilibrium constant, K, for a redox reaction is related to the standard cell potential, Ecel, by the equation Reduction half-reaction (V) Ag+ (aq) + e-→Ag(s) Cu2+ (aq) + 2e-→Cu(s) 0.34 Sn (a) 4e-Sn(s 0.15 2H' (aq) + 2e-→H2 (g) Ni2+ (aq) + 2e-→Ni(s)-0.26 Fe2+ (aq) + 2e-→Fe(s)-0.45 Zn2+ (aq) + 2e-→Zn(s)-0.76 Al3+ (aq) +3e-→Al(s) -1.66 Mg2+ (aq) + 2e-→Mg(s) -2.37 0.80 n FEcell where n is the number of moles of electrons...
Table 3: Experimental Data for Part 2: Determination of Activation Energy k Time* T* [1] [S,0,?]...
Table 3: Experimental Data for Part 2: Determination of Activation Energy k Time* T* [1] [S,0,?] Rate (M/s) (s) (C) (M) (M) Run 3 153 20.5 .0208 .0416 4.03*10^-6 4.65*10^-3 (Room T) Run 6 198 9 .0208 .0416 3.15*10^-6 3.64*10^-3 (Cool) Run 7 112 31 .0208 .0416 5.58*10^-6 6.45*10^-3 (Warm) Run 8 40 51 .0208 .0416 1.56*10^-5 1.80*10^-2 (Warmer) 1/T (1/K) In k Run 3 1/293.5 -5.37 Run 6 1/282 -5.62 Run 7 1/304 -5.044 Run 8 1/324 -4.02 20....
Effect of Temperature on Cell Potential Cell designation: E (measured) Temperature (°C) PbPb2+ || Cu2+ Cu; 0.455 Temperature (K) AG (calculated) 0.497 295 0.512 Sn Sn2+ || Cult | Cu; 0.548 0.554 279 295 0.566 343 Y AS determined from the slope of a plot of AG versus T AS Pb Cur AS Sn|Cu = AH° Pb | Cu=- AHSn Cu=- AHº calculated at 298 K (show calculations) from AG = AH-TAS AH = AG+TAS
Electrochemical Cells and Thermodynamics Key (calculated) Shorthand cell designation ΔΟ (calculated) E cell (measured) Temperature ( ) and Keq for an exemplary pair. For Pb | Pb2+ Isn2+ Sn: Show calculations for E half-cell (calculated) Half-cell equation Effect of Temperature on Cell Potential Cell designation: E (measured Tempegature fc) Temperature (kK) AG (calculated) 5 c 1134 228 K 2315 AS determined from the slope of a plot of AG versus T (show calculations) AfP calculated at 298 K 233
Electrochemical...
Ive
attacthed all my results. I just need help calculating question 4
and 5
(5 pts) Part II. Your experimental data: how many sig figs should your temperature data have? Show work for one calculation of temp in Kelvin. Show work for one AG calculation: Approximate Measured Cell Calculated Temp (°C) Calculated Temp (°C) potential Temp (K) AG Ecell (V)* (kJ/mol)* * measured value 70.21 0.581 343 1-112.1 65.12 0.680338 - 111.9 Show work: 60.02 0.5715333 -1110 °C -> 5.05+278.15...
equation in graph: E=1.13E+00-1.08E-04T
8. (10 pts) A cell is constructed Cu2+ to Cu, while the zinc is oxidized from Zn to Zn+. The cell potential is measured as temperature, yielding the graph below. with a copper anode and a zinc cathode. The copper is reduced from 1 3E-00-1.08E-04 T e» 1 8 280 290 300 310 320 330 340 350 Determine Δrrn // and ΔrrnS for this reaction from the data given.
8. (10 pts) A cell is constructed...
Can someone please help me finish the tables and
calculations.
Thanks in advance
Data Sheet Part A: Dependence of Reaction Rate on Concentration Table 1 H Temperature Time Relative mixture ! (seconds) | rate 1000 Reaction BrOsl (eC) . 1235.6 Avg. time 2. 67.S 3. 08,24 Avg. time 2. 74.2 3. 70.74.O Avg. time 24.o' 4 弘·11 0.2 OD3 0.00 8 100 o.oy | 23.5 3. 29. Avg. time 교 Table 2: Calculations for the [I']. [Bro, & [H'] BrOs...
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
Partner's Name Instructor Procedure I, Voltaic Cell Zn/Zn2+ 1.0 M || Cu2+ 1.0 M/Cu In the space below write the equations for the two half reactions and sum them appropriately to calculate the standard reaction potential for a 1.0 M voltaic cell. Show the overall net ionic equation for this reaction. 9pts.) Standard reaction potential Write the expression for Q for this redox reaction. (4 pes) In the space below show a calculation using the Nemst equation to determine the...
how
do I solve this?
1. Use the Nernst equation to calculate the standard cell potential for a voltaic cell of a Sn electrode in 0.10M Sn2(a) in one half-cell and Al in 0.10M AP) in the other. (EPe Eaode- Emode 1.52 V, Show your work. Hint: Check E values of the reduction haif reactions. Write the one with more negative E as oxidation half reaction (change the sign); ensure that equal number of electrons are exchanged ie. electrons cancel,...
Cell Potential and Equilibrium Standard reduction potentials The equilibrium constant, K, for a redox reaction is related to the standard cell potential, Ecel, by the equation Reduction half-reaction (V) Ag+ (aq) + e-→Ag(s) Cu2+ (aq) + 2e-→Cu(s) 0.34 Sn (a) 4e-Sn(s 0.15 2H' (aq) + 2e-→H2 (g) Ni2+ (aq) + 2e-→Ni(s)-0.26 Fe2+ (aq) + 2e-→Fe(s)-0.45 Zn2+ (aq) + 2e-→Zn(s)-0.76 Al3+ (aq) +3e-→Al(s) -1.66 Mg2+ (aq) + 2e-→Mg(s) -2.37 0.80 n FEcell where n is the number of moles of electrons...
Table 3: Experimental Data for Part 2: Determination of Activation Energy k Time* T* [1] [S,0,?] Rate (M/s) (s) (C) (M) (M) Run 3 153 20.5 .0208 .0416 4.03*10^-6 4.65*10^-3 (Room T) Run 6 198 9 .0208 .0416 3.15*10^-6 3.64*10^-3 (Cool) Run 7 112 31 .0208 .0416 5.58*10^-6 6.45*10^-3 (Warm) Run 8 40 51 .0208 .0416 1.56*10^-5 1.80*10^-2 (Warmer) 1/T (1/K) In k Run 3 1/293.5 -5.37 Run 6 1/282 -5.62 Run 7 1/304 -5.044 Run 8 1/324 -4.02 20....
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