PS-1. BioenergeticsIn photosynthesis, the following processes are happening:- O2 + 4H* + 4e- CH2O + H2O2H2OCO2 + 4H* + 4e -CO2 + H2O → CH2O+O2Find the total expenditure of energy required in order to produce one molecule of CH2Ofrom CO2 and H2O?standard redox potential of H2O - O2 pair is -0.82 Vstandard redox potential of CO2 - CH2O pair is -0.4 V

During the process of photosynthesis, carbon dioxide is reduced to glucose and water is oxidized to…

Answered: PS-1. Bioenergetics In photosynthesis,…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.4QAP

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Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 3.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (c) Is the reaction spontaneous at a pH of 8.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M and all gases at 1.00 atm?
Consider the reaction below at 25°C: 2MnO4(aq)+16H+(aq)+10Br(aq)2Mn2+(aq)+5Br2(l)+8H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 2.00 with all other ionic species at 0.100 M? (c) Is the reaction spontaneous at a pH of 5.00 with all other ionic species at 0.100 M? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M?
What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
In theory, most metals should easily corrode in air. Why? A group of metals called the noble metals are relatively difficult to corrode in air. Some noble metals include gold, platinum, and silver. Reference Table 17-1 to come up with a possible reason why the noble metals are relatively difficult to corrode.
Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a pH meter at 25 00C is given by the equation where contains the potential of the reference electrode and all other potentials that arise in the cell that are not related to the hydrogen ion concentration. Assume that = 0.250 V and that a. What is the uncertainty in the values of pH and [H+] if the uncertainty in the measured potential is 1 m V ( 0.001 V)? b. To what precision must the potential be measured for the uncertainty in pH to be 0.02 pH unit?
The free energy change for the following reaction at 25 °C, when [H+] = 1.14 M and [Cr3+] = 5.01×10-3 M, is -442 kJ:6H+(1.14 M) + 2Cr(s)3H2(g) + 2Cr3+(5.01×10-3 M) ΔG = -442 kJWhat is the cell potential for the reaction as written under these conditions?____________ VWould this reaction be spontaneous in the forward or the reverse direction?
Ozone (O3) and chlorine dioxide (ClO2) are both strong oxidizing agents. Given the half reactions for these species as follow: O3 + 2H+ + 2e- = O2 + H2O, E0 = 2.07 V vs. SHE ClO2 + e- = ClO2-, E0 = 1.15 V vs. SHE Write and balance the overall reaction that occurs when O3 is mixed with NaClO2 in aqueous solution. What is the standard Gibbs free energy for the overall reaction?
I want all questions answered Consider the cell: Pt|H₂(g,p°)| HCl(aq)|AgCl(s)|Ag for which the cell reaction is 2AgCl(s) +H₂(g) → 2 Ag(s) + 2HCl(aq). At 25 °C and a molality of HCl of 0.010 mol kg⁻¹ . Calculate ionic strength of solution?Calculate (in volts) Standard Electrode Potential of the cell E°:?Calculate (in kJ/mol) Standard Gibbs Free Energy of the cell ΔrG°?Assuming Debye-Huckel limiting law holds at this concentration, calculate (in volts) Ecell (Cl⁻, AgCl, Ag)? Assuming Debye-Huckel limiting law holds at this concentration, calculate (in kJ) ΔrG?
The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.11 M and [Cr3+] = 3.59×10-3 M, is -638 kJ:3Cu2+(1.11 M) + 2Cr(s) → 3Cu(s) + 2Cr3+(3.59×10-3 M) ΔG = -638 kJWhat is the cell potential for the reaction as written under these conditions?Answer: ____ VWould this reaction be spontaneous in the forward or the reverse direction?

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