d. A redox reaction with an electron stoichiometry n = 3 has a reaction quotient Q...
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....
If the equilibrium constant for a two-electron redox reaction at 298 K is 1.4×10−4, calculate the corresponding ΔG∘ and E∘cel under standard conditions.
D Question 14 3 pts The following redox reaction is conducted with [A13+] = 0.80 M and [Mn2+] = 0.30 M. 2 Al(s) + 3 Mn2+(aq) + 2 A13+(aq) + 3 Mn(s) Ecell = 0.48 V Determine the moles of electrons transferred for the reaction as written (n), Q, and the cell potential (cell) at 298 K. n= (Select] Q = (Select] Ecell = (Select)
Redox : If members of the redox couples above were used to set
up the most energetically favorable chemical
reaction, the initial electron donor should be
___and the final electron acceptor should be
___.
Use the information from the redox couples below to answer the fill in the blank questions, using the letter after each substance. (i.e. if you believe that the answer is CoQ fill in the appropriate blank with the letter A). Each letter (substance) may be used...
A two electron redox reaction has a redox potential E' = 0.58 V. Given Faraday's constant F = 96,500 J/mol, calculate the standard Gibb's free energy change AG in kJ (to three significant figures) for the reaction.
0/1 point Calculate the value of the reaction quotient, Q. for the galvanic cell expressed using shorthand notation below. Use the balanced chemical equation that has the smallest, whole number stoichiometric coefficients. Znis) 224. 0.0100 M) Aglaq, 1.25 M) Ais Agʻlag) e Agte) +0.80 V Znagl + 2 e Zn(s) E".0.76 V * 8.00 x 10-3 125 156 6.40 x 10-3
QUESTION 4 A balanced redox reaction involves exchange of 2 electrons and generates a potential difference of 1 V under standard conditions. What is the equilibrium constant for the reaction? A. 192 В. 6.41x 1033 С. 1.56 x 10-34 D.2.0 E. 96485
please show work
Balance the chemical equation for the following redox reaction under basic aqueous conditions with the smallest whole-number coefficients possible using the half-reaction method. How many moles of electrons are transferred in the balanced reaction? N, 0(g) + C10,- (aq) → CIO" (aq) + NO, (aq) d. 18 b. 6 e. 24 c. 12 a. 4 Calculate AG" for an electrochemical cell reaction that occurs under acidic aqueous conditions based on the following two half-reactions for which the...
Redox: The best initial electron donor for an
organism performing fermentation would be ___, while the best final
electron acceptor would be ___ .
Use the information from the redox couples below to answer the fill in the blank questions, using the letter after each substance. (i.e. if you believe that the answer is CoQ fill in the appropriate blank with the letter A). Each letter (substance) may be used more than once. Hint: put the redox couples into an...
At 58.0 ∘C , what is the maximum value of the reaction quotient, Q, needed to produce a non-negative Ecell value for the reaction SO42−(aq)+4H+(aq)+2Br−(aq)⇌Br2(l)+SO2(g)+2H2O(l) In other words, what is Q when Ecell=0 at this temperature? I found that Ecell = 0.87 V and n= 2 −nF(Ecell−E∘cell) / 2.303RT = 2×96485 (0+0.87)/2.303×8.314×331.0 log q = -26.49 I need Q without log