Effect of Temperature on Cell Potential Cell designation: E (measured) Temperature (°C) PbPb2+ || Cu2+ Cu;...
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 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...
Show calculations for the half cell equations that i put
please.
Shorthand cell designation Temperature () E cell (measured) AG (calculated) K (calculated) 78 2. -78 3. Show calculations for AG® and Kg for an exemplary pair. For Pb) Pb2 ISn2 IS: Half-cell equation E half-cell,(calculated) 24- 2+
Part B: Cell Potential and Temperature (Pb/Cu cell) 1. Fill in the table. Use cell one sample calculation. Don't forget the units! se your measured cell potential to calculate E and AG at each temperature. Show Temp CTemp (K)E (measured) E° 32.2 30S. 3 481 m 42, 3 |31 S, SDI 482 2.3 B3S,4S 88 Use Excel to create a graph of AG (y-axis) vs Temperature (K) (x-axis). Insert a linear trendline. 2. Report the ungeneralized trendline equation and R2...
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...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...
please help the standrad reduction provided down
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 9.24x10 + M and the Cr3+ concentration is 1.47 M? 3Cu2+ (aq) + 2Cr(s) Answer: 3Cu(s) + 2Cr +(aq) v The cell reaction as written above is spontaneous for the concentrations given: What is the calculated value of the cell potential at 298K for an electrochemical cell with the...
Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Mg2 ] = 0.774 M and [Sn2 ] = 0.0190 M. Standard reduction potentials can be found here. Reduction Half-Reaction Standard Potential Ered° (V) F2(g) + 2e– → 2F–(aq) +2.87 O3(g) + 2H3O+(aq) + 2e– → O2(g) + 3H2O(l) +2.076 Co3+(aq) + e– → Co2+(aq) +1.92 H2O2(aq) + 2H3O+(aq) + 2e– → 2H2O(l) +1.776 N2O(g) + 2H3O+(aq) + 2e– → N2(g) + 3H2O(l) +1.766 Ce4+(aq) + e– → Ce3+(aq)...