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Please ASAP. Thank you.
Calculate Equilibrium/Reversal Potentials of Sodium and Potassium ions.
[Na+]outside =165 mM
[Na+]inside =15 mM
[K+]outside =16 mM
[K+]inside = 220 mM
Temperature, T = 37 = (37 + 273.15) K = 310.15 K
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Solved in 4 steps
- The following cell was found to have a potential of 0.2897 V:SCEIIMg2+(a = 3.32 * 10^-3M)membrane electrode for Mg^2+(a) When the solution of known magnesium activity was replaced with an unknown solution, the potentialwas found to be 0.2041 V. What was the pMg of this unknown solution?(b) Assuming an uncertainty of 60.002 V in the junction potential, what is the range of Mg21 activitieswithin which the true value might be expected?(c) What is the relative error in [Mg^2+] associated with the uncertainty in Ej?5) a) Typical Mg²+ concentrations in blood plasma are 2.2mM. If the transmembrane po- tential across the cell membrane is -90mV (negative inside), calculate the equilibrium con- centration of Mg²+ inside the red blood cell at 37°C. b) Consider the difference in electrochemical potential inside vs outside the cell, Aµreleefchem Helece/chem (inside) – Helec/chem(outside). As discussed in class, this difference is written as a chemical and electrical contribution, Afdee/chem = Aflchem + Atelec: For the red blood cell at equilibrium, state whether Atelee/chem; Atchem, and Aftelec are greater than, less than, or equal to zero, and explain your answer.a) Chlorine is disproportionate in basic medium. And in an acid medium? Write both reactions and calculate the final potential, indicating if they are thermodynamically favorable (See Frost diagram) ClO- /Cl2 = 0.42 V HClO /Cl2 = 1.63 V Cl2 /Cl- = 1.36 V b) Use the Latimer diagram of chlorine in acid medium to determine the potential corresponding to the reduction of ClO4 - to Cl2. Write the fitted equation of this reaction.
- 2) A 90.00 ml solution, density = 1.0582 g/mL. with a AG = specif ic heat of 4.079 J/(GC), increased in temperature ΔΗ- from 20.36 C to 28.13 t with Al added. The copper collected, weighed 2.087 g. The electrochemical AS = potential mean was +1.821 volts. Calculate AG AH and AS for the reaction below. +3 2A (aq) +2 2 Als) * 3 Cuaq) 3 C46)(Q93) What is the value of ECELL (in V) for the following unbalanced reaction: Mg2+ (aq) + Al (s) ---> Mg (s) + A1³+ (aq) when it occurs at 25°C and the concentrations of the species are as follows: [Mg2+] = 0.151 M [A1³+] = 4.82 x 10-5 M The reduction potentials for the two half-reactions involved are: Mg2+ + 2 e---> Mg (s) (E°RED) = -2.37 V Al³+ + 3 e- --> Al (s) (E°RED) = -1.66 V (Please give me four decimal places - if Canvas will allow - so that it is easier for me to award partial credit as appropriate).1. A Cr3+ solution is electrolyzed using a current of0.365 A. What mass of Cr(s) (51.9661) is plated outafter 10 hours?2. When an aqueous solution of CuSO4 is electrolyzedcopper metal is deposited. If a constant current waspassed for 5.00 h and 404 mg of Cu (63.546) metal wasdeposited, what was the current?
- The standard potentials for the couples Pb2+/Pb and Pb4+/ Pb²+ is +1.8 V and -0.126 V, respectively. Would there be an expectation of Pb²+ to disproportionate in aqueous solution? And why?Calculate the equilibrium potential for a neuron at 26 °C using the concentration given [K +]o =5mM [CI - Jo =100 mM [Na +]o =145mM [K +]j =130 mM [CI - ]; =8 mM [Na +]j =5mMCalculate the potential of a platinum electrode immersed in a solution that is (a) 0.0613 M in K4Fe(CN)6 and 0.00669 M inK3Fe(CN)6. E0=0.36 (b) 0.0400 M in FeSO4 and 0.00915 M in Fe2(SO4)3. E0=0.771 (c) buffered to a pH of 5.55 and saturated with H2 at 1.00 atm. (d) 0.1015 M in V(OH)4+, 0.0799 M in VO2+, and 0.0800 M in HClO4. E0=1 (e) prepared by mixing 50.00 mL of 0.0607 M Ce(SO4)2 with an equal volume of 0.100 M FeCl2 (assume solutions were 1.00 M in H2SO4 and use formal potentials).E0=0.68 (f ) prepared by mixing 25.00 mL of 0.0832 M V2(SO4)3 with 50.00 mL of 0.00628 M V(OH)4+ and has a pH of 1.00.
- In a polarographic experiment of a 60 mL of 0.08 M Cu2+solution, a limitingcurrent was left on for 15 minutes. If the average current during the time of theexperiment is 6.0 μA, what fraction of the copper is removed from the solution? TheFaraday constant is 96485 C/mol of electron.An aqueous solution of SO2 reduces (a) aqueous KMnO4 toMnSO4(aq), (b) acidic aqueous K2Cr2O7 to aqueous Cr3 + ,(c) aqueous Hg2(NO3)2 to mercury metal. Write balancedequations for these reactions.How long would it take (in minutes) to reduce 1 mole of each of the following ions using the current indicated? (Ampere (A) = Coulomb/second (C/s), I = C/s, F= 96500 C/mol e-) (C = Charge unit Coulomb, n = electron mole number) Q=I×t=n×F(a) Fe3+ , 2.344 A (b) Cu2+ , 25.260 A