coagulation-1

Calculate the cell potential of a cell operating with the following reaction at 25°C in which [Cr2O72] = 0.040 M , I] = 0.025 M, [Cr**] = 0.10 M, and [H*] = 0.45 M. %3D Cr2 O,2 (ag) + 6I (aq) + 14H+ (aq) → 2Cr³+ (aq) + 3I2 (s) + 7H2O(1) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E° (V) I2 (s) + 2e = 21 (aq) 0.54 Cr2 O,2 (aq) + 14H† (aq) + 6e¯ = 2Cr** (aq) + 7H2O(1) 1.33 Cell potential = V

Homework: 1- Determine the thermodynamic tendency for silver to corrode in a aerated acid solution at pH = 1.0 Assume = a Ag+ = 10° and Pm = latm , and Po2 = 0.2atm compare the result to that of Example 1 ( deaerated solution ), [ERg/Ag+= 799 mv]

please help me

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Procedure: Add 0.1M H2O2 and several drops of 6M H2SO4 to 0.1M KI. Observation: Solution goes from a light amber to a dark, dark Blue.   H2O2(aq) + 2KI(aq) + H2SO4(aq) → I2(s) + K2SO4(aq) + 2H2O(l) Has oxidation and reduction occurred? If oxidation and reduction has occurred? If oxidation and reduction has occurred define the change in oxidation numbers for the following atoms and define what is undergoing oxidation and reduction:   I[ ? ] → I[ ? ] O[ ? ] → O[ ? ]

Ex 14. Will magnesium shavings dissolve if added to an aqueous solution of ferrous sulphate? Justify your answer! Mg2+/Mg = -2,714 V; ºFe2+/Fe = -0,44 V a/ Yes, because Mg is a stronger oxidant than Fe b/ Yes, because Mg is a stronger reducer than Fe c/ No, because Mg is a weaker reducer than Fe d/ No, because Mg is a weaker oxidant than Fe Ex 15. Determine the type of each of the electrodes depending on the type of potential-determining ions and write down the Nernst equation for calculating their electrode potential: a) Ag/AgCl, KCl b) Pt, H₂/HCl (a=1). c) Fe/Fe(NO3) d) Pt/Co²+,Co³+. Justify your answer!

Q.5.A Q5.B

4 - 7. A voltaic cell is constructed using the following half-reactions: Cu*(ag) + e -> Cu(s). ɛ° = +0.521 V 1216) + 2e¯ -> 21 (aq) ɛ° = +0.536 V The cell is operated at 298 K with [Cu*] = 2.1 M and [1] = 3.2 M 5. Which electrode is the anode of the cell? O A. Cu*/Cu2+ B. Cu/Cu* C. Cu/Cu2+ O D. I'/l2

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Question 2 ELECTROCHEMISTRY: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous solution containing M2X3 (where X is the anion) with a supplied current of 6.86 A for 9 h, and consumes 0.1573 kWh of electrical energy. Assume that the current efficiency is 80%. Input values only with 2 decimal places. Do not include the unit. Round your answer to 2 decimal places.

= to Write balanced half-reactions for the following redox reaction: 2+ 2 MnO4 (aq)+8 H₂O()+10 Cl(aq) > 2 Mn (aq) + 16 OH (aq)+5 Cl₂(g) osoft O ELECTROCHEMISTRY Writing the half-reactions of a complex redox reaction in acidic ... rosoft 2.210... reduction: oxidation: 0 Explanation Check 9,211 J 121 Q 103 NOV 1 #tv ♫♬ C202-0020 Chara B C 2022

TUTOR Voltaic Cells Under Non-Standard Conditions Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.033 M at 25 °C. 2 Fe2"(aq) + H2O2(aq) + 2 H"(aq) → 2 Fe"(aq) + 2 H,O(E) Acidic Solution Standard Electrode Potential, E°(volts) H2O2(aq) + 2 H'(aq) + 2 e →2 H2O(E) Au*(aq) + e – Au(s) Au3 (aq) + 3 e →Au(s) +1.77 +1.68 +1.50 Br2(t) + 2 e -→2 Br(aq) +1.08 NO3 (aq) + 4 H'(aq) + 3 e → NO(g) + 2 H20 +0.96 Ag*(aq) + e –Ag(s) Hgz2"(aq) + 2 e →2 Hg(8) Fe (aq) + e--→ Fe²"(aq) Cu2"(aq) + 2 e → Cu(s) +0.80 +0.789 +0.77 +0.337 HgzClz(s) + 2 e →2 Hg(t) + 2 C(aq) Sn**(aq) + 2e → Sn2*(aq) +0.27 +0.15 2 H*(aq) + 2 e →H2(g) Pb?*(aq) + 2 e → Pb(s) 0.00 -0.126 Sn2*(aq) + 2 e → Sn(s) Ni2"(aq) + 2 e → Ni(s) Cd2*(aq) + 2 e → Cd(s) Cr**(aq) + e – Cr**(aq) Fe2"(aq) + 2 e → Fe(s) Zn2"(aq) + 2 e → Zn(s) Cr2*( aq) + 2 e → Cr(s) A* (aq) + 3 e Mg2*(aq) + 2 e → Mg(s) -0.14 -0.25 -0.40 -0.408 -0.44 -0.763 -0.91 Al(s) -1.66 -2.37

ANSWER PLEASE HUHU A 100.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of 25.00-mL of 0.00250 M K2Cr2O7 resulted in the reaction 6Fe2+ + Cr2O7 2- + 14H+ → 6Fe3+ + 2Cr3+ + 7H2O The excess K2Cr2O7 was back-titrated with 9.40 mL of 0.00951 M Fe2+ solution. Calculate the concentration of iron in the sample in parts per million.

4 - 7. A voltaic cell is constructed using the following half-reactions: Cu*(aq) + e -> Cu(s) ɛ° = +0.521 V I2(s) + 2e" -> 21 (aq) ɛ° = +0.536 V The cell is operated at 298 K with [Cu*] = 2.1 M and [I'] = 3.2 M 6. Is the answer in no. 5 the same as it would be if the cell were operated under standard conditions? A. No O B. Yes O C. Cannot be determined

Consider 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 V

III Writing the half-reactions of a complex redox reaction in acidic... Write balanced half-reactions for the following redox reaction: 6 Cl₂(9)+C₂H₂OH()+3H₂O() 12 Cl(aq)+2 CO₂(g)+12H* (aq) reduction: oxidation: Explanation Check COMPLETE & CONTINUE → MacBook Pro ローロ 9₁ X 00 S 2022 McGraw Hill LLC. All R

Please correct answer and don't used hand raiting

Consider the following cell reaction: Fe(s) + 2 H*(? M) –→FE²*(1.00 M) + H»(g)(1.00 atm) If the cell potential at 298 K is 0.280 volts, what is the pH of the hydrogen electrode? pH =| %3D Submit Answer Retry Entire Group 4 more group attempts remaining

Show work..don't give Ai generated solution

Please give me fast answer and expat answer solutions

1.3. Write the half-cell reactions for each of the following cells:a). Ag∣Ag+∥H+∣H2∣Ptb). Pt∣Cr2O–27,Cr+3,H+∥Br–∣Br2(l)∣Pt

I don't understand what the xM is or how to find [H+]

Can you make an electrochemical cell by placing a silver electrode in 1.00 L of 4 g AgI (Ksp = 3´10-17) solution and a zinc electrode in 1.00 L of 6 g ZnCl2 (pKsp =  - 5.11) solution. If yes, what will be the initial voltage of this cell.

Task 1: Determine the standard reduction potential of the fictional metals Vibranium (Vb/Vb2+) and Adamantine (Ad/Ad*) using the partial table of standard cell potential data given below. Entries marked with 'x' were not measured. Standard Cell Cathode Potentials, E°cell (V) Vb/Vb2+ Cu/Cu2+ Ad/Ad* Ag/Ag+ Mg/Mg2+ Pt/H2/H* Vb/Vb2+ Cu/Cu²+ Ad/Ad* Ag/Ag* Mg/Mg2+ Pt/H/H* 0. + 2.114 + 0.896 0. + 1.218 - 1.218 X + 3.155 0. + 2.370 + 0.337 Standard reduction potential of Vb/Vb²+ = V Standard reduction potential of Ad/Ad* = V Anode

When pH = 7, p(O2) = 100 kPa,   //check picture //  calculate the electrode potential in according to the reaction.

4 - 7. A voltaic cell is constructed using the following half-reactions: Cu*(ag) + e -> Cu(s) ɛ° = +0.521 V 121s) + 2e -> 21(ag) ɛ° = +0.536 V The cell is operated at 298 K with [Cu*] = 2.1 M and [I'] = 3.2 M 4. Determine ɛ for the cell at these concentrations. O A. 0.015V B. -0.015V O C. 0.034V D. 0.0076V

A10.00 solution 0.050M of AgNO3 was titrated with 0.0250 M of NaBR using an calomel electrode. ( E= 0.241) Find the voltage of the cell when: 0.1ml, 10.00ml, 20.00ml and 30.00 ml of titrant is added. Ag+ + Br- --> AgBr (s) Ag+ + e- ---> Ag(s)   ( E= 0.799) Use this reaction for Nerst equation   Ksp= 5.0x10^-13

4. a. 18.00 mL of 0.125 M Sn++ is titrated with 0.100 M Ti²+, according to the reaction: Sn+ + Ti²+→→ Sn²+ + Ti³+ Find: a) Erxn [0.522 V] b) the equivalence point volume of Ti²+ [45.00 mL] b. What is the reduction potential, Ern, of the solution above when the volume of added Ti²+ is: a) 15.00 mL? [0.163 V] b) 22.50 mL? c) 45.00 mL? d) 60.00 mL? e) 90.00 mL? [0.154 V] [-0.020 V] [-0.0340 V] [-0.368 V]