Using the Nernst equation [E=E degree cell- (-.0592/n) log Q], calculate the cell potential if [Cr3+] = 0.10M and [Cu2+]= 0.0010M. E degree cell = -1.08V
Using the Nernst equation [E=E degree cell- (-.0592/n) log Q], calculate the cell potential if [Cr3+]...
Use the Nernst equation to calculate the theoretical value of E of th copper-concentration cell and compare this value with th cell potential you measured. E = E* - 0.0592 / n * logQ **So I believe this is the equation that I would use. However, i'm don't know what E* is suppose to be...** The my electrochemistry experiment the cell potential that i measured were: 0.130V, 0.115V, and 0.110V (average cell potential = 0.118V) The concentration of the copper...
Using the Nernst equation, calculate the cell potential for the following reaction (T=298 K): Cr2O72- (aq) + 14 H+ (aq) 6 I- (aq) → 2 Cr3+ (aq) + 3 I2 (s) + 7 H2O (l) given that Cr2O72- = 1.7 M H+ = 1 M I- = 1 M Cr3+ = 0.002 M
Choose the correct Nernst equation for the cell Zn + Cu2+ à Zn2+ + Cu E = E° - 0.0296 log(Cu / Zn) E=E° - 0.059 log([Zn2+] / [Cu2+]) E = E° - 0.0296 log(Zn / Cu) E = E° - 0.0296 log([Zn2+] / [Cu2+]) E = E° - 0.0296 log([Cu2+] / [Zn2+]) 20 points
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,...
Electrochemical cell potential can be calculated using the Nernst equation. $$ E_{\text {cell }}=E_{c \text { cell }}^{o}-\left(\frac{R T}{n F}\right) \ln Q $$ Identify the value represented by each variable in the equation. Ecell: Choose... El Choose... R: Choose... T: Choose... n: Choose... F: Choose... Q: Choose...
III O ELECTROCHEMISTRY Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr + (aq) +3Ca (s) -- 2Cr (s) +3Ca²+ (aq) 2+ Suppose the cell is prepared with 0.699 M Cr3+ in one half-cell and 6.35 M Ca? in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 미미 X ? Check
use the nernst equation to calculate the theoretical value of E of the copper concentration cell and compare this value with the cell potential that you measured DATA TABLE Results of Parts I and II Cu/Pb X/Pb Y/Pb 0.431 0.172 0.581 Average cell potential (V) Results of Part III Cu concentration 0.042 Average cell potential (V)
The cell potential of a redox reaction occurring in an electrochemical cell under any set of temperature and concentration conditions can be determined from the standard cell potential of the cell using the Nernst equation where E is the cell potential of the cell, E° is the standard cell potential of the cell, R is the gas constant, T is the temperature in kelvin, n is the moles of electrons transferred in the reaction, and Q is the reaction quotient....
For the cell schematic below, identify values for n and Q, and calculate the cell potential, Ecell. Al(s)│Al3+(aq,0.15M)║Cu2+(aq,0.025M)│Cu(s)
The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is Part A E E- 2.303 RT logO For the reaction nF 2C03 (aq)2Ci (aq)+2C02+ (aq) Cl2 (g). E = 0.483 V where E is the potential in volts, E° is the standard potential in volts, R is the gas constant, T what is the cell potential at 25 °C if the concentrations are Co3+ M, and the...