CHEM N-12 November In the electrolytic production of Al, what mass of Al can be deposited in 2.00 hours by a current of 1.8 A?

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1 CHEM N-1 November 014 In the electrolytic production of Al, what mass of Al can be deposited in.00 hours by a current of 1.8 A? What products would you expect at the anode and the cathode on electrolysis of a 1 M aqueous solution of NiI? Explain your answers.

2 CHEM N-13 November 014 An electrochemical cell is consists of 1.0 L half-cells of Fe/Fe + and Cd/Cd + with the following initial concentrations: [Fe + ] = M, [Cd + ] = 0.00 M. What is the initial E cell at 5 C? 8 What is E cell when [Cd + ] reaches 0.15 M? What is [Cd + ] when E cell reaches V? What are the equilibrium concentrations of both ions? [Cd + ] = [Fe + ] =

3 CHEM N-11 November 013 What is the electrochemical potential of the following cell at 5 o C? Fe FeSO 4 (0.010 M) (FeSO 4 (0.100 M) Fe 3 Calculate the mass of aluminium which can be produced with the same quantity of electricity that is used to produce 1.00 kg of copper metal. Explain why Na(s) cannot be obtained by the electrolysis of aqueous NaCl solutions.

4 CHEM N-11 November 01 A galvanic cell consists of a Cr 3+ /Cr half-cell with unknown [Cr 3+ ] and a Ni + /Ni halfcell with [Ni + ] = 1.0 M. The electromotive force of the cell at 5 C was measured to be 0.55 V. What is the concentration of Cr 3+ in the Cr 3+ /Cr half-cell? 6 Calculate the equilibrium constant of the reaction at 5 C. Calculate the standard Gibbs free energy of the reaction at 5 C. Express the overall reaction in the shorthand voltaic cell notation.

5 CHEM N-1 November 01 A strip of copper and a strip of zinc are embedded in a lemon, and are connected by wires to a voltmeter; a voltage is generated and can be read at the voltmeter. What chemical reactions are occurring that lead to the generation of current? 3 Assuming there are no losses in the circuit and the conditions are similar to standard, what voltage can be read at the voltmeter?

6 CHEM N-13 November 01 A 0.0 ml sample of 0.11 M Fe + in an acid solution was used to titrate 3.5 ml of a KMnO 4 solution of unknown concentration. Write the balanced redox reaction that occurs in solution upon titration, and calculate the molarity of the KMnO 4 solution. 4

7 CHEM N-10 November 010 How many minutes would be required to obtain 10.0 g of liquid mercury by passing a constant current of 0.17 A through a solution containing Hg (NO 3 ) (aq)? Page Total:

8 CHEM N-11 November 010 Calculate ΔG for the following reaction: 3Cu(s) + Cr 3+ (aq) 3Cu + (aq) + Cr(s) 3 Is the reaction spontaneous under standard conditions? Give a reason for your answer. THE REMAINDER OF THIS PAGE IS FOR ROUGH WORKING ONLY. Page Total:

9 CHEM N-15 November 009 The standard reduction potential of phosphorous acid to hypophosphorous acid is V, with the following half-reaction: H 3 PO 3 (aq) + H + (aq) + e H 3 PO (aq) + H O(l) What would the reduction potential be for this half reaction at a temperature of 5 C in an aqueous solution with ph of.3 and concentrations of [H 3 PO 3 (aq)] = 0.37 M and [H 3 PO (aq)] = M? 3 A number of bacteria can reduce the nitrate ion in the presence of sulfur. A simplified unbalanced redox reaction can be written as: S(s) + NO 3 (aq) SO (g) + NO(g) Balance this redox equation for acidic conditions.

10 CHEM N-16 November 009 What is the value of the equilibrium constant for the following reaction at 98 K? Fe 3+ (aq) + 3Sn(s) Fe(s) + 3Sn + (aq) Relevant electrode potentials can be found on the data page. 3

11 CHEM N-9 November 008 A galvanic cell is made of a Zn + /Zn half cell with [Zn + ] =.0 M and an Ag + /Ag half cell with [Ag + ] = M. Calculate the electromotive force of the cell at 5 C. 5 Calculate the equilibrium constant of the reaction at 5 C. Calculate the standard Gibbs free energy of the reaction at 5 C. Indicate whether the reaction is spontaneous or not. Give a reason for your answer. Express the overall reaction in the shorthand voltaic cell notation.

12 CHEM N-11 November 008 A melt of NaCl is electrolysed for 35 minutes with a current of 3.50 A. Calculate the mass of sodium and volume of chlorine at 40 C and 1.00 atm that are formed. 4

13 CHEM N-13 November 008 A concentration cell containing aqueous solutions of Cu(NO 3 ) and solid copper metal is constructed so that the Cu + ion concentration in the cathode half-cell is 0.66 M. Calculate the concentration of the Cu + ion in the anode half-cell if the cell potential for the concentration cell at 5 C is 0.03 V. In acid solution, dichromate ion oxidises iron(ii) to iron(iii) as illustrated in the partial equation: Fe + + Cr O 7 Fe 3+ + Cr 3+ Write a balanced equation for this reaction. 3 What would happen to the cell potential if the concentration of Cr 3+ were increased?

14 CHEM N-10 November 007 How many minutes would be required to electroplate 5.0 g of manganese by passing a constant current of 4.8 A through a solution containing MnO 4?

15 CHEM N-11 November 007 The solubility product constant of AgCl is K sp = M. Using the relevant electrode potentials found on the data page, calculate the reduction potential at 98 K of a half-cell formed by: (a) an Ag electrode immersed in a saturated solution of AgCl. 6 (b) an Ag electrode immersed in a 0.5 M solution of KCl containing some AgCl precipitate. Each of these half-cells is connected to a standard Cu + (1 M)/Cu(s) half-cell. In which half-cell, (a) or (b), will clear evidence of a reaction be seen? Describe the change(s) observed.

16 CHEM N-10 November 006 The physiological properties of chromium depend on its oxidation state. Consider the half reaction in which Cr(VI) is reduced to Cr(III). CrO 4 (aq) + 4H O(l) + 3e Cr(OH) 3 (s) + 5OH (aq) E o = 0.13 V Calculate the potential for this half reaction at 5 o C, where ph = 7.40 and [CrO 4 (aq)] = M. 3

17 CHEM N-11 November 006 Consider the following reaction at 98 K. Ni + (aq) + Zn(s) Ni(s) + Zn + (aq) Calculate G o for the cell. (Relevant electrode potentials can be found on the data page.) 5 What is the value of the equilibrium constant for the reaction at 98 K? Express the overall reaction in voltaic cell notation. Using a current of.00 A, how long (in minutes) will it take to plate out all of the silver from 0.50 L of a M Ag + (aq) solution?

18 CHEM N-1 November 006 Calculate the standard free-energy change for the following reaction at 98 K. Au(s) + 3Mg + (1.0 M) Au 3+ (1.0 M) + 3Mg(s)

19 CHEM N-8 November 005 Calculate the standard free-energy change for the following reaction at 98 K. Au(s) + 3Ca + (1.0 M) Au 3+ (1.0 M) + 3Ca(s) Complete and balance the following equation for the reaction between iron(ii) ions and permanganate ions in an acidic solution. Fe + + MnO 4 Fe 3+ + Mn + What is the value of the equilibrium constant for the following reaction at 98 K? Fe 3+ (aq) + Sn(s) Sn + (aq) + Fe + (aq)

20 CHEM N-8 November 004 Consider the following balanced redox reaction. In(s) + 3MnO (s) + 1H + (aq) In 3+ (aq) + 3Mn + (aq) + 6H O If E o = V, what would be the measured potential of this cell at 98 K at the following concentrations? [H + (aq)] = 0.5 M; [In 3+ (aq)] = 0.0 M; [Mn + (aq)] = 0.4 M What is the value of the equilibrium constant for the following reaction at 98 K? Cu + (aq) + Zn(s) Zn + (aq) + Cu(s) Relevant electrode potentials can be found on the data page.

21 CHEM J-8 June 003 Consider the following half-reactions and their standard reduction potentials. ClO 3 + 1H e Cl + 6H O E = 1.47 V S O 8 + e SO 4 E =.01 V Give the overall cell reaction. 3 Calculate G and hence the value of K c for the cell reaction at 98 K. G = K c =

1.In which of the following is the oxidation number of the underlined element given incorrectly? oxidation number

General Chemistry II Exam 4 Practice Problems 1 1.In which of the following is the oxidation number of the underlined element given incorrectly? oxidation number a. K 2 Cr 2 O 7 +6 b. NaAl(OH) 4 +3 c.