1. Write the following balanced reactions using cell notation. Use platinum asan inert electrode, if needed.a. Mns) + Sn(N03)2(aq)Mn(NO3)z(aq) + Au(s)b. 3CUNO3(aq) + Au(NO3)3(aq) 3Cu(NO,)z(aq) + Aus)2. Given the following cell notations, determine the species oxidized, speciesreduced, and the oxidizing agent and reducing agent, without writing thebalanced reactions.) b. Nic) I Niag) Agiag) I Ag()a. Mg I Mgaq)I Cu ag) I Cus)2+ag) Agiag) I Ags)3. For the cell notations in the previous problem, write the correspondingbalanced reactions.

Here we have to write the cell notation of the following redox reactions. For this we have to know…

1. Write the following balanced reactions using cell notation. Use platinum as an inert electrode, if needed. a. Mns) + Sn(NO3)2(aq)M b. 3CUNO3(aq) + Au(NO3)3(aq) Mn(NO3)2(aq) + Au(s) 3Cu(NO,)z(aq) + Au(s)

1. Write the following balanced reactions using cell notation. Use platinum as an inert electrode, if needed. a. Mns) + Sn(NO3)2(aq)M b. 3CUNO3(aq) + Au(NO3)3(aq) Mn(NO3)2(aq) + Au(s) 3Cu(NO,)z(aq) + Au(s)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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2. Write the cell notation and cell diagram; and identify which is in anode and cathode. a. Ag+(aq) + Mg(s) ----> Ag(s) Mg(s) b. AgcI(s) + Fe(s) -----> Ag(s) + Fe+2(aq) + Cl- (aq) c. Fe(s) + H+(aq) -----> Fe+2(aq) + H2(g,1atm) d. Pb+2(aq) + Cr+2(aq) -----> Pb(s) + Cr+3(aq) e. Au+3(aq) + Fe+2(aq) -----> Au(s) + 4 Cl-(aq) + Fe+3(aq) f. K+(aq) + H2O(I) ----> 02(g) + H+ (aq) + K(s) a. Ag'ia + Mg --> Ag Mg b. AgClos + Fe -----> Aga) + Fe* + Clua) c. Fe + H'ag) > Fela + Hae latm d. Pb" + Cr e. Au f. K'ua + HOn > On + H'aa) + Ko --> Pb + Cru -> Au + 4 Cl n) + Fe" + Fe 2. For the above item #1, a-f; write the cell notation and cell diagram; and identify which is in anode and cathode.
11. What is AG° for the reaction driving the following voltaic cell? Co (s) | Co²+ (aq) || Mn³+ (aq), Mn²+ (aq) | Pt (s) A. -175 kJ +175 kJ B. -351 kJ +351 kJ C. -527 kJ D. E.
2. The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum? d. If the electronic charge is 1.60 x 10-¹C, what is the total electrical charge used? e. If a constant current of 90 mA were applied, what was the time elapsed in seconds and in minutes?
3. write a report on the use of zinc as a “sacrificial anode” to minimise the corrosion of iron and steel such as on ships. Use the standard electrode potentials given in question 2 above to predict the cell emf and overall equation for the reaction that would occur in standard conditions between zinc and iron. With ocean-going ships, however, what is the solution in which the two metals are immersed? Is this solution always at an exact concentration of 1 mol dm-3? And in what ways does this real-life situation differ from the standard condition of 25oC / 298K Picture of question 2 is also given
A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb+2 half cell. All solutions are 1.0 M. Ag+(aq) + e- → Ag(s) E° = 0.80 V Pb+2(aq) + 2e- → Pb(s) E° = -0.13 V a.Diagram the cell, labeling electrodes and solutions, show the direction of electron flow in the circuit and what occurs in the salt bridge. b. If the cell were made with [Pb+2] = 0.10 M and [Ag3+] = 3.0 M, would the voltage increase, decrease, or remain the same? Explain using Q. c.Identify the electrode that is gaining mass
Cr(s) Cr(NO3)3 A Voltaic Cell NaCl(aq) Pb(s) Pb(NO3)2 Cr³+ (aq) + 3 eCr (s) E° = -0.41 V Pb²+ (aq) + 2 e¯¯ → Pb (s) E° = -0.12 V The concentration of the solutions in each half-cell is 1.0 mol/L. Placing some Cr(s) in a solution containing Pb2+ ions. Placing some Pb(s) in a solution containing Cr³+ ions. O Placing some Cr(s) in a solution containing Cr³+ ions. O Placing some Pb(s) in a solution containing Pb³+ ions. Based on the given reduction potentials, which of the following would lead to a reaction?
35. Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction as set up. 4F⁻(aq) + Mn2+(aq) → 2F2(g) + Mn(s) F2(g) + 2e⁻ → 2 F⁻(aq) E° = +2.87 V Mn2+(aq) + 2 e⁻ → Mn(s) E° = -1.18 V A) 1.69 V B) 4.05 V C) -4.05 V D) +2.87 V
Zn(s) + 2 H*(aq) → Zn²*(aq) + H2(g) 1. What is the effect on the cell potential of a voltaic cell wi h the above reaction when: The pressure of H2 gas is increased in the cathode. c. Sodium hydroxide is added to the cathode half-cell decreasing the [H"]. а. b. Zinc nitrate is added to the anode d. The surface area of the anode is doubled. half-cell.
A student contructs an electrochemical cell consisting of a silver electrode in a 0.10 M solution of AgNO3 connected through a salt bridge to a zinc electrode in a 0.10 M solution of Zn(NO3)2. The potential across the electrochemical cell was measured as 1.52 V. a. Write the half reactions for the cathode and the anode. b. Use standard notation to represent this electrochemical cell.
8. NA KNO3(aq) salt bridge Z(s) T 1.0 MZ(NO3)₂ (aq) 1.0 MX(NO3)₂(aq) Half-Reaction X (aq)+2e →X(s) Z²+ (aq) + 2 e → Z(s) X(s) Standard Reduction Potential (V) -1.25 V 0.45 V Consider the voltaic cell, half-reactions, and standard reduction potentials shown above. Which reaction occurs at the anode?
11. The following two half-cells are connected to form a full Galvanic cell: Cu"(aq) +2e Au (aq) +e → Cu(s) → Au(s) E° = 0.34 V E 1.69 V a. Calculate E° for the cell. b. Give the cell notation for this system. c. Give the balanced cell reaction. d. Calculate AG for the reaction e. Calculate Keg for the reaction. £. Calculate the cell potential if the activity of Cu is 0.0100 and the activity of Au" is 1.340.
9. A voltaic cell is constructed using the following: Fe (s) + 2H* (aq) -> H2 (g) + Fe (aq) a. What is the potential under standard conditions? b. What is the potential when [Fe2] = 1.25 M, P2 = 1.15 atm, and the pH in both cells is 4.75 at 298 K? C. What is the Gibb's Free Energy and the equilibrium constant, K under standard conditions? What are these values with the conditions of part b? Did the reaction become more or less spontaneous? Explain.