For the cell: pt/ Hz cratmy / NaOH cm)/ Hg0 cs) / Hq Ezask, -0.924V o-854V and 298 Catcutate standard electromotive force ES ge write the eleetrods reaAions and the Cett reaetion So calculate the eleetromotive foree at 308 K 298 K when the change in inthalpy (AH) = 35 kcal to Cell reaction aud, what happen to electromotive force when added few amount of nitric acid to equivalent to the base NaOH partially 2
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- The Nernst-Planck equation (shown below) describes the motion of a charged chemical species in a fluid. dC; z,FC; dv J; = - D; dx RT dx' What are the units for the ion flux J, where: zis the valence state of the ion (unitless) C is the concentration (mol/m³) Fis the Faraday constant (Coulomb/mol) Ris the ideal gas constant (kg m²/(s² mol °K)) Tis the temperature (K) dCi/dx is the concentration gradient (mol/m*) dV/dx is the electric potential gradient (V/m) D; is the diffusion coefficient (m²/s) Note that Coulomb is a unit of charge and V is volts where 1 V= 1 Joule/Coulomb)The electrometive force of the half cells at 2s čs -08V Ag / Ag Ag/ Ag Br -0.071V calculate: Solubility producct constant to silver bromide 2 O electromotive force Ag/AgBress/ HBr co.021)/Hefe atm}/ pt when the efficiency Coefficient to hydcogen bromide to the Celle o-9Research has been conducted on molybdates as replacements for chromates in the surface treatment of various metals in order to reduce corrosion by the formation of a surface film of MoO,. The overall reaction with iron is 2Fe(s) + 3M00- (aq) + 6H*(aq) - Fe;Os(s) + 3M0O:(s) + 3H;O() Given the following AG; in calories per mole at 25°C: Fe,O; (s) =-177,100, MoO:(s) =-120,000, H:O (1) =-56,690, Mo0; (aq) =-205,420 (a) Is the above overall reaction spontaneous under standard conditions? (b) Calculate the standard electrode potential for the above overall reaction. (c) Write an expression for the electrode potential as a function of molybdate ion concentration and pH. (d) Is the overall reaction spontaneous for a molybdate ion concentration of 0.001M at pH 7.0?
- A galvanic cell ZatNZa"tag) Co"(agCe) is constructed using a completely immersed Za electrode that weighs 31.8 g and a Ce electrode immersed in 671 ml. of 1.00 M Co" (ag) solution. A steady current of 0.0793 A is drwn from the cell s the electrons move from the Zn electrode to the Co electrode. (a) Which reactant is the limiting reactant in this cell? Eer ymbel b) How long does it take for the cell so be completely discharged? (e) How much mass has the Co clectrode gained when the cell is completely discharged (4) What is the concentration of the Ca"(ag) when the cell is completely discharged? (Assume that the limiting reactant is 100s reacted) M Dutnt Anwer fusumu dur uonenbsA piece of an unknown weighing 12.50is placed in 49.7cm of water in a cylinder. The water level increases to 69.0cm3. whats the calculated value for the drnsity of the solid in g ml-1Oc. 12 L O d. 18 L Clear my choice n 8 How many Faraday is needed to deposit 6.0 moles of Sn from SnCl43 ed О а. 12.00 out of Оь. 24.00 uestion O c. 6.00 O d. 18.00 Determine the molality of a solution in which 5.3 grams of glucose C12H22011 are dissolved in 1484grams of water.
- The electromotive force of the half cells at 25čs Ag / Ag Ag / Ag Br -0.071V Solubility producct constant to silver bromide ? O electromotive force calculate: to the Celle Ag/AgBress/ HBr co.02M)/Hafe atm}{ pt when the efficiency Coefficient to hydrogen bromideQ. 5. (a) A KCI solution having N/50 normality has specific conductivity equal to 0.0102. If K* and Cl ions have ionic conductance of are 43.0 and 65.0 ohm' at the same temperature individually, determine the degree of dissociation of KCI solution. (b) A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate solution (4M). Calculate the molarity of the solution at the end of electrolysis. (c) 0.02 M CH3COOH solution has a resistance of 240 ohm with a cell constant of 0.366 cm'. Calculate the degree of dissociation and dissociation of CH3COOH at 0.02 M concentration. Given A° HCI, NaCl, CH3COONA are 435, 138 and 99 scm? mol respectively.5.25 Consider a hydrogen electrode in HBr(aq) at 25°C operating at 1.45 bar. Estimate the change in the electrode potential when the solution is changed from 5.0 mmol dm3 to 25.0 mmol dm³.
- enow.com/ilrn/takeAssignment/takeCovalentActivity.. A 电 | [Review Topics] Use the References to access important values if needed for this question. For the reaction 2HB1(g)H2(g) + Br2(1) oHV AHo = 72.6 kJ and AS° = -114.5 J/K The equilibrium constant for this reaction at 283.0 K is Assume that AH° and AS° are independent of temperature. Submit Answer Retry Entire Group 2 more group attempts remaining (Previous Save and Exit Cengage Learning | Cengage Technical Support 10:03PM 72°F 4/11/2022 VNCStandard Reduction (Electrode) Potentials at 25 Half-Cell Reaction * (volts) F2(8) + 2 e2F (aq) 287 Ce* (aq) +e Ce (aq) 1.61 Mn0, (aq) + BH'(aq) +5e Mn"( "(aq) + 4 H20(1) 1.51 Cla(g) +2e -2 C (aq) 1.36 Cr20, (aq) + 14 H'(aq) - 6e2 Cr*"(aq) + 7 H20() 1.33 Oz() + 4 H'(aq) + 4e2 H20(1) 1.229 Br20) + 2 e2 Br (aq) 1.08 NO3 (aq) + 4 H'(aq) + 3eNO(g) + 2 H20() Hg"(aq) 0.96 2 Hg (aq) + 2e 0.920 Hg"(aq) + 2 e- Hg(1) 0.855 Ag (aq) +e Ag(s) 0.799 Hg2" (aq) - 2e-2 Hg(1) 0.789 Fe" (aq) +e Fe"(ag) 0.771 12(s) + 2e 21 (aq) 0.535 Fe(CN)"(aq) + e Fe(CN), (aq) 0.48 Cu (aq) + 2eCu(s) 0.337 Cu"(aq) +e- Cu (aq) 0.153 S(s) + 2 H'(aq) + 2 e H2S(aq) 0.14 2H'(aq) + 2e-H2(8) 0.0000 Pb (aq) + 2e- Ph(s) -0126 Sn (aq) + 2 e Sn(s) -014 Ni (aq) + 2 e- Ni(s) -0.25 Co (aq) + 2 e Co(s) -0.28 "(aq) + 2e Cd(s) -0.403 Cr"(aq) +e "(aq) -041 Fe"(aq) + 2 e Fe(s) -044 Cr"(aq) +3e-Cr(s) -0.74 Zn"(aq) +2 e- Zn(s) -0.763 2 H20() +2e Hz(z) + 2 OH (aq) -0.83 Mn"(aq) + 2e - Mn(s) -1.18 A" (aq) + 3e- Al(s) -1.66 Mg (aq) + 2 e- Mg(s)…www-awn.aleks.com scgi/x/Ist.cxe/1o u-lgNslkr7j8P3H-1JITX1655270TVADBLZzfZ TTDXW2 e5N8WY11OPcLAKYDH7EWSASLm O ELECTROCHEMISTRY Recognizing consistency among equilibrium constant, free.. ON A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG". • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E". His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred pei redox reaction is 2. calculated quantities (Check the box next to any that are wrong.) cell AG" K E" A. 226. kJ/mol 39 3.92 x 10 -1.17 V В 224. kJ/mol 1.75 x 10…