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- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.
- Use the following data to calculate the enthalpy of solution of sodium perchlorate, NaClO4: fH(s)=382.9kJ/mol and fH(aq,1m)=369.5kJ/molTable 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.Determine the equilibrium constant for the reaction Sn+Pb2+Sn2++Pb
- 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 Gibbs energy for a reaction Mg(s) + H₂O(g) → MgO(s) + H₂(g) at a particular temperature is AG = -100.0 kJ/mol. At the same time under the sa conditions, A,G° = +341 kJ/mol. Which of the following statements is true? The reaction is at equilibrium and P(H₂O) = P(H₂). The reaction proceeds in the reverse direction to produce more H₂O(g). The reaction proceeds in the forward direction to produce more H₂(g). The reaction is at equilibrium and P(H₂O) > P(H₂). The reaction is at equilibrium and P(H₂O) < P(H2).Gibbs energy change, A¡G° , is related to cell potential, Eell, by the equation A;G° = –nFEel Part B where n is the number of moles of electrons transferred Calculate the standard cell potential at 25 ° C for the reaction and F = 96 500 C mol1 is the Faraday's constant. X(s) + 2Y*(ag)→+X²+(ag) +2Y(s) where A,H° = -675 kJ mol1 and A,S° = -393 J K-1 mol-1 Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) ? HA Value Units %3D cell Submit Previous Answers X Incorrect; Try Again
- Consider the following reaction and standard cell potential:N2H4(aq) + O2(g) → N2(g) + 2H2O(I)E°cell = 1.56 VUnder standard conditions, what is the change in Gibbs free energy (AG°) in units of kJ for this reaction?AG°=-nFEF = 96.485C / m * ol1A = 1 C/sec1V = 1J / CType your answer...Consider the cell, Zn(s)|ZnCl2(0.0050 mol kg−1)|Hg2Cl2(s)|Hg(l), for which the cell reaction is Hg2Cl2(s) + Zn(s) → 2 Hg(l) + 2 Cl−(aq) + Zn2+(aq). The cell potential is +1.2272 V, E⦵(Zn2+,Zn) = −0.7628 V, and E⦵(Hg2Cl2,Hg) = +0.2676 V. (a) Write the Nernst equation for the cell. Determine (b) the standard cell potential, (c) ΔrG, ΔrG⦵, and K for the cell reaction, (d) the mean ionic activity and activity coefficient of ZnCl2 from the measured cell potential, and (e) the mean ionic activity coefficient of ZnCl2 from the Debye–Hückel limiting law. (f) Given that (∂Ecell/∂T)p = −4.52 × 10−4 V K−1, Calculate ΔrS and ΔrH.