The Nernst EquationA nonstandard cell or half-cell potential can be calculated using the Nernst equation:RTE = E° -InQnFwhereE = potential under nonstandard conditionsE = standard potentialR = ideal gas constant = 8.314 J/K mol%3D%3DT = kelvin temperaturenumber of moles of electrons for the reaction aswrittenF = charge carried by 1 mol of electrons =96, 485 C/mol = 96, 485 J/V · mol%3D= reaction quotient%3DIt is customary to use the equation in a form where numberical values are substituted for R, T, and F at a temperature of 25° C.(8.314 J/K - mol)(298K)96, 485 J/V molRT= 0.02568 VFand the Nernst equation with the potentials in volts is:E = E° –0.02568In QSometimes it is more convenient to use base-10 logarithms, and the substitution of 2.3026 log for In is made.(2.3026 x 0.02568 = 0.0591)%3DE = E0.0591logQ–A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correctlogarithm.=- EEUEU Tor this question.What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu+concentration is 1.16 M and the Zn concentration is 3.83 x 10¬ M ?Cu?+ (aq) + Zn(s) → Cu(s) + Zn²+ (aq)EcellVThe cell reaction as written above isfor the concentrations given.spontaneousSubmit AnswerRetry Entire Groupnonspontaneouspts remaining

Given that, a cell reaction is Cu2+aq + Zns →Cus + Zn2+aq. The concentrations are [Cu2+] = 1.16 M…

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu+ concentration is 1.16 M and the Znt concentration is 3.83 x 10 M? Cu* (aq) + Zn(s) → Cu(s) + Zn+ (aq) Ecell V The cell reaction as written above is v for the concentrations given. spontaneous nonspontaneous Submit Answer Retry Entire Group pts remaining

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu+ concentration is 1.16 M and the Znt concentration is 3.83 x 10 M? Cu* (aq) + Zn(s) → Cu(s) + Zn+ (aq) Ecell V The cell reaction as written above is v for the concentrations given. spontaneous nonspontaneous Submit Answer Retry Entire Group pts remaining

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

us the tabulated half cell potentials to calculate ▲G° for the following redox reaction 2Al(s) + 3Mg2+(aq) --> 2Al3+(aq) +3Mg(s)
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag* concentration is 6.38×10 4 M and the Zn2* concentration is 1.17 M ? 2+ 2Ag*(aq) + Zn(s)- →2Ag(s) + Zn²*(aq) Answer: V The cell reaction as written above spontaneous for the concentrations given:
eq Preq 1req F2 # 3 LU E D What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Pb²+ concentration is 8.54 x 10-4 M and the Mg2+ concentration is 1.23 M ? Ecell F3 The cell reaction as written above is Submit Answer $ SA 4 2+ Pb²+ (aq) + Mg(s) → Pb(s) + Mg²+ (aq) R F V V F4 % References] Use the References to access important values if needed for this question. стор T Retry Entire Group G DII Cengage Learning Cengage Technical Support F5 OL Y H F6 9 more group attempts remaining & 7 U ✓for the concentrations given. F7 J OO PrtScn BN M F8 K Home F9 L End F10 Previous PgUp F11 Next Save and Exit 4x10 PgDn 8:28 PM 12/2/2022 F12 1 Ins {
What is the calculated value of the cell potential concentration is 1.13M, and the Ag* concentration is 1.33M ? 298K for an electrochemical cell with the following reaction, when the F2 pressure is 1.73×10-4 atm, the F F2(g) + 2Ag(s)– →2F*(aq) + 2Ag*(aq) Answer: The cell reaction as written above is spontaneous for the concentrations given: ( true Submit Answer Retry Entire Group 9 more group attempts remaining
When the Ag* concentration is 1.33 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 3.279V. What is the Mg?+ concentration? 2Ag*(aq) + Mg(s)- →2Ag(s) + Mg²*(aq) Answer: M
When the Hg*+ concentration is 1.35 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.143V. What is the MIN2+ concentration? Hg* (aq) + Mn(s)→ Hg(1) + Mn²"(aq) Answer: M
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 8.22×10-4 atm, the F concentration is 1.46M, and the Cr³+ concentration is 1.01M? 3F₂(g) + 2Cr(s)—6F¯(aq) + 2Cr³+ (aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: