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- At 25C, you conduct a titration of 20.00 mL of a 0.0400 M AgNO3 solution with a 0.050 M NaI solution within the following cell: Saturated Calomel Electrode | Titration solution | Ag(s) for the cell as writted, what is the voltage after the addition of 10.00 mL of the NaI sooution? The reduction potential for the saturated calomel electrode is E=0.241 V. The standard reduction potential for the reaction: Ag++e- ® Ag(s) E0= 0.79993V. The solubility constant of AgI is Ksp=8.3x10-17 Note: the cell potential could be negative since the condditions are non-standard ones. a)0.169 b)0.354 c)0.235 d)2.360 e)0.441Consider a ring which was electroplated with gold (Au, MM = 197 g/mol) using an Au(III) salt with a 0.328-Ampere current for 4.00 min. R= 8.314 J/mol-K; F = 96,485 J/mol-V 1. How much electric charge passed through the cell? [Select] V II. How many moles of electrons passed through the cell? [Select] III. How much gold were deposited onto the ring? [Select] V V3. A precipitate of AgCl + AgBr weighs 0.8132 g. On heating on a current of Cl2, the AgBr is converted to AgCl, the mixture loses 0.1450 g in wt. Find the percentage Cl in the original sample.
- ELECTROCHEMISTRY: Copper was electroplated from a Cu2S04 solution onto an electrode with an active surface area of 6.49 cm2. Determine the thickness (mm) of the deposit if the current is kept constant at 3.48 A for 1.3118 hours. (density of Cu = 8.96 g/cm3, MW of Cu = 63.55 g/mol). (Input values only with 2 decimal places. Do not include the unit.)Given the standard of the Cu2+/Cu and the Cu+/Cu couples are +0.340 V and +0.522 V, respectively, evaluate E°(Cu2+/ Cu+)Given the following half-reactions Mn2+(aq) + €2- -› Mn(s); E°= - 1.18 V Cu2+(ac) + €2- -Cu(s): E° = 0.34V Cr-0-2-(aq) + 14H*(aq) + €6- - 2Cp+ (aq) + 7H20(1); E° = 1.33V select the best reducing agent.
- 目 4. Given the schematic notation: Cu | Cu2* (0.0200 M) || Ag* (0.0200 M) | Ag, calculate the cell D. Focus PsIn a Zn|ZNSO4||CuSO4|Cu cell where both solutions are clear and NOT colored, adding equimolar Zn2* to the Cu/CUSO4 setup will make the reaction (spontaneous/nonspontaneous/not work) . This is becauseELECTROCHEMISTRY: Copper was electroplated from a Cu2S04 solution onto an electrode with an active surface area of 4.31 cm?. Determine the thickness (mm) of the deposit if the current is kept constant at 3.04 A for 1.0784 hours. (density of Cu = 8.96 g/cm3, MW of Cu = 63.55 g/mol). (Input values only with 2 decimal places. Do not include the unit.)
- 3+ half cells ave 10- Ered. for Fe/ Fe and Fe / fe -o-44V and ten 77 ¥ be the Vatue of E for Fel Fe half cell2 respectivelythen what Eox- 3+ willGiven the following half reaction: b. Pt| Fe".Fes c. Zn|Zn2 d. Ag|Ag For each of the following cell combination and or conditions (where the negative electrode is at the left of the combination). Combination A: a and b Combination 8:cmeasured against a salurated calomel electrode at 30°C Combination C: b and d Combination D: c and aif ( = 1.20M and (Zn] = 0.80M at 25°C Determine anode half reaction, cathode half reaction, overall reaction, cell notation, cell potential, free energy change, spontaneity and the equilibrium .constant. The equilibrium constant is related to the standard cell potential through: RT In K nF20. Due to COVID-19 coupled with erratic power supply from ZESCO, you decide to play around with galvanic cells and you construct a zinc-copper battery operating at a zero resistant small light emitting diode (L.E.D) at 25°C as follows: Zn | Zn²*(0.10 M) || Cu2* (2.5 M) | Cu The mass of each solid electrode is 2.00 g. a) b) c) Which of the two is a reducing agent? Calculate the cell potential when this battery is first connected. Calculate the cell potential after 10.0 A of current has flowed for 10.0 hours. (Assume each half-cell contains 1.00 L of solution.) d) e) Calculate the mass of each electrode after 10.0 hourS. What will cause the battery to die after some time? o search hp f7 f8 f9 f10 f11 f12 f3 米 f4 IOI f5 C f6 www 73 1 & 7 7 8. $ 2 3 5 8 € 6 E R T Y U P S D F G K V B 88 TECNO SPARK at gr 00 堂