Pb2+(aq) + 2 e → Pb(s) Br2(0) + 2 e* → 2 Br(aq) E° = -0.13 V E° = +1.07 V

Q: A solution is prepared by dissolving 22.7 g of Al2(S04)3 in water. What current would be needed to…

A:

Q: Determine the value of the formation constant ( K;) for AUCI4, using the correct combination of the…

A: Given reactions are    Au3+ (aq) + 3 e-  ------> Au(s)                                 Eo =1.52 V…

Q: Calculate the E for the following equation. Use these standard potentials. Fe(s)+F₂(g) →→→→ Fe²+…

A: Standard cell potential is determined by :  E°cell = (E°RP)cathode - (E°RP)Anode  At cathode…

Q: How much time (in hours to two decimal places) must pass to produce 50 grams of gold using a 6.50 A…

A: Use the given quantities carefully to solve for time taken by gold.

Q: The standard reduction potentials for two pairs of redox species are shown below. Which species is…

A: Answer: Cu+1(aq) Explanation:  The one which is having more standard reduction potential (SRP) value…

Q: The

A: We can observe the table. Mg has less reduction potential than Fe.

Q: For the following electron-transfer reaction: 3Cl₂(g) + 2Cr(s) →→→→ 6Cl¯(aq) + 2Cr³+ (aq) The…

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Q: Calculate Current or Time How many amperes are required to deposit 0.242 grams of silver metal in…

A:

Q: Please answer letter D, E and F. See attached pic.

A: electro chemical series         Mn+2     -1.182        Cd+2       -0.402        Pb+2      -0.13…

Q: Consider the following standard reduction potentials Ag+(aq)   + e-→Ag(s)…

A:

Q: Determine E° for the half-reaction In3 (aq) + 3 e' → In(s). 2ln(s) + 6H*(aq) → 2ln3+(aq) + 3H2(g) E°…

A: The standard EMF of a galvanic cell is given as= Standard EMF of cell= standard EMF of cathode +…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Recall the given redox reaction,                           We have to calculate the standard…

Q: Standard Reduction Potentials F₂(g) + 2e2F (aq) Cl(g) + 2e-2Cl(aq) Cu (aq) + 2e Cu(s) Pb (aq) + 2e-…

A: Oxidation is defined as increase in oxidation state of the element and reduction means decrease in…

Q: Use the half-reactions shown below to answer the following questions. Half-reaction |E° (V) Br2(1) +…

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Q: Consider the following half-reaction containing acid HX below.   3 N2(g) + 2 H+(aq) + 2 e-  →  2 HX…

A: given:  O3(g) + 2 H+(aq) + 2 e-  →  O2(g) + H2O (l)  E°red = 2.076 V   find: Could HX be applied to…

Q: Consider these two entries from a fictional table of standard reduction potentials. x+(aq) + e →…

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Q: Met (aq)+N(s) - N+ (aq) + M(s)' The standard reduction potentials are: M+ (aq) + ae M(s) e =0.400 V…

A: The given half reactions are The Nernst equation for (1) is The Nernst equation for (2) is For…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Data

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: The given redox reaction is 2NOg + 2H2Ol + Br2l →2HNO2aq + 2H+aq + 2Br-aq. We have to calculate the…

Q: Consider the following standard reduction potentials: Fe3+ (aq) + e MnO4 (aq) + 8 H*(aq) + 5e → Mn2+…

A: In this question, we will see the strongest oxidizing agent.  You can see below.

Q: What current must be supplied to deposit 4.77 g of gold from a solution of AuCl 3 in 27.2 min?

A:

Q: Cr³+ (aq) + e → Cr²+ (aq) 2H(aq) + 2e → H2(g) E° = -0.41 V E° = 0 V

A: Given:  ECr3+|Cr2+o=-0.41 VEH+|H2o=0 V

Q: What is Eᵒ(cell) for the reaction 2 Au(s) + 3 Ca²+(aq) → 2 Au³+(aq) + 3 Ca(s)? Standard Reduction…

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Q: What current (in A) is required to plate out 1.92 g of magnesium from a solution of Mg in 3.60 x 10…

A: Given is Solution of Mg+2 ions, and 1.92g  Mg is deposited in 3.60×103 seconds. Current = ?

Q: Which species would act as the cathode in the following reaction? ​ 4 Au(s)  +  16 Cl-(aq)  +  3…

A: in  electrochemical cell reaction, one species is oxidized and other species is reduced.

Q: NO2–1    (aq) +  I -1    (aq)® NO (g) + I2(s)  Oxidation numbers for every atom  Oxidation and…

A: Some rules to be followed while calculating oxidation number: 1) Oxidation number of oxygen atom is…

Q: a. Under standard-state condițions, which is the strongest oxidizing agent? [ Select ] b. Under…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: All of our standard reduction potentials are supposed to be at "standard acidic conditions, which…

A:

Q: Co³*(aq) + e¯ → Co²*(aq) → Fe²+(aq) E° = +1.953 V Fe*(aq) + e¯ E° = +0.769 V %3D I;(aq) + 2e¯ –→…

A: Since we only answer up to 3 sub parts, we'll answer the first 3. Please resubmit the question and…

Q: E°(V). -1.66 3+ + 3e¯→ Al(s) +0.07 gBr(s) + e¯→ Ag(s) + Br¯ 4+ + 2e → Sn 2+ +0.14 ° 3+ + e¯→ Fe2+…

A: Loss of electrons is oxidation.  Gain of electron is reduction. Species undergo oxidation is…

Q: Reduction half-reaction E* (V) 2 H2O(£) + 2 e¯ → H2 (g) + 2 OH (aq) H2 (g) + 2 OH¯(aq) -0.83 Sn+…

A: Which is more eaily reduced ?

Q: V³+ (aq) + e¯ → V²+ (aq) Sn+ (aq) + 2e →→ Sn²+ (aq) 4+ E° = -0.255 V E° = +0.154 V

A: E0(V3+) = -0.255 VE0(Sn4+) = 0.154 VR = 8.314 J/molKT = 298K

Q: Using the standard electrode potentials: Cl₂(g) +2e-2Cl(aq) E° = +1.36 V; Cd2+ (aq) + 2e → Cd(s) E°…

A: Standard electrode potential is given.  According to electrode potential in electrochemical series,…

Q: Using the standard electrode potentials: Cl2(g) + 2e 2CI (aq) E° = +1.36 V; Cd2*(aq) + 2e- Cd(s) E°…

A: In the electrochemical cell, the chemical energy is converted into electrical energy. The addition…

Q: 9. Which line notation correctly represents each electrochemical cell?…

A:

Q: Write the overall chemical reaction and calculate E° for the following reduction and oxidation…

A: The half reactions taking place are, Reduction : 2 H+ (aq) + 2 e- -----> H2 (g)…

Q: From the standard reduction potentials given below, which of the following pairs of substances will…

A: We know for a reaction to be spontaneous,  must be negative. We also know -So in order to be…

Q: Identify which of these metals, if coated onto iron, would prevent the corrosion of iron. Check all…

A: In corrosion of iron, Fe in presence of oxygen oxidized to Fe2O3. xH2O.  This is also known as…

Q: A2 + 2e → 2A- E° = +1.09 V D2+ + 2e → D E° = -2.37 V

A: Oxidising agent is that substance which oxidises other compounds and gets itself reduced easily.

Q: Given the following standard reduction potentials, E°red, which species has the  greatest tendency…

A: In an electrochemical cell, the electrode with a higher standard reduction potential acts as a…

Q: Determine E° for the reaction: Mg(s) + Sn⁴⁺(aq) → Mg²⁺(aq) + Sn²⁺(aq) Reduction half-reaction:…

A: The gain of electrons is known as reduction. The loss of electrons is known as oxidation.

Q: current of 2.505 A deposits 1.371 g of a metal M from a solution that contains the metal ion M²⁺ in…

A: Given, current (i) = 2.505 A Time (t) = 30 × 60 = 1800 s Mass = 1.371 g  Using Faraday's law,  Mass…

Q: How many hours are required to produce 795 grams of lead from molten lead(II) chloride (PbCl2, 278.1…

A:

Q: Which species of the following half-reactions will reduce Pb +2(aq)? I2(s) + 2 e- → 2 I-(aq) E° =…

A: ->The specie which has greater reduction potential (with sign) that tends to reduce itself and…

Q: Consider the following reduction half-reactions: MnO4 (aq) + 8 H*(aq) + 5 e¯ = Mn²+ (aq) + 4H₂O(1)…

A:

Q: Which of the following substances is the strongest oxidizing agent?

A: Oxidizing agent are substances which reduces itself and oxidizes other species.

Q: Calculate Keq for the following redox reaction using the information provided: 3 E2+(aq)  + 2 Z (s)…

A: The relation between standard cell potential and equilibrium constant is as follows,…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.