Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- How many hours is required to plate 25.00g of copper metal from 1.00 M CuSO4(aq) by using a current of 3.0 A
Use Faraday's Law. Answer: 7.0h
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- Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive) layer of a precious metal, such as silver or gold. In essence the metal object is made the cathode of an electrolytic cell in which the precious metal cations are dissolved in aqueous solution. Suppose a current of 0.320 A is passed through an electroplating cell with an aqueous solution of AgNO3 in the cathode compartment for 10.0 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol. ロ・ロ X μ olo Sarrow_forwardHow many moles of hydroxide ion will be produced at the cathode during the electrolysis of water with a current of 4.52 A for a period of 2.77 minutes? The cathode reaction is 2H₂O + 2e → H₂ + 2OH- mol OH = =arrow_forwardHow many grams of silver can be plated onto an object in 7.46 minutes at 3.07 A of current? Ag+ (aq) +e → ► Ag(s) Your Answer: Answer unitsarrow_forward
- An aqueous FeF₂ solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Half-reaction at anode: Half-reaction at cathode: + + Standard Reduction Potentials (Volts) at 25 °C 2 F (aq) F₂(g) +2 e 2.870 O₂(g) + 4 H3O*(aq) + 4 e¯ →→ 6 H₂O(l) 1.229 2 H₂O(1) +2 eH₂(g) + 2 OH(aq) -0.828 Fe²+ (aq) + 2 e Fe(s) + (b) What is the expected decomposition potential? -0.440 +arrow_forwardA certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell apparatus is filled with a 225. mM solution of MNO3 and the right half cell with a 4.50 M solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. x10 Which electrode will be positive? left right X Ś ? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.arrow_forwardWhat mass of material will be deposited at the cathode when a current of 10.5 A is applied for 2.0 hours to the following cell: Cr(s) | Cr² (aq) || Al*(aq) | Al(s)arrow_forward
- Consider the following galvanic cell: Li (s) | 0.095M LiCl (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s) Using Appendix H in the textbook, determine the Ecell of this galvanic cell. 2.54 V - 2.88 V O -2.92 V 2.88 V 2.92 Varrow_forwardA certain metal è forms a soluble sulfate salt ₂(so). Suppose the left half cell of a galvanic cell apparatus is filled with a 5.00 M solution of M₂(SO4)3 and the right half cell with a 250. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. Which electrode will be positive? O left Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. O right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 x10 Xarrow_forwardNonmetallic phosphorus can be made by the electrolysis of molten P4010. (a) What mass of P is formed by passing a current of 8.60 A through molten P4010 for 1.30 days? The unbalanced chemical reaction representing this electrolysis is shown below. g of P is formed by this electrolysis. (b) How many minutes are needed to plate out 14.00 g of P from molten P4010 using 8.97 A current? minutes are needed. P4010 → P + 0₂arrow_forward
- How many grams of silver can be plated onto an object in 16.28 minutes at 7.54 A of current? Ag+ (aq) +e → ► Ag(s) Your Answer: Answer unitsarrow_forwardCalculate the cell potential of a cell composed of a cathode consisting of a Co wire immersed in a 1.44 M Co²+ solution and an anode consisting of a Co wire immersed in a 5.60×10-5 M Co²+ solution. Assume the temperature of the solutions is 298 K. Cell potential: Varrow_forwardMetallic nickel can be made by the electrolysis of molten NiCl₂. (a) What mass of Ni is formed by passing a current of 7.09 A through molten NiCl₂ for 4.70 days? The unbalanced chemical reaction representing this electrolysis is shown below. NiCl₂ → Ni + Cl₂ g of Ni is formed by this electrolysis. (b) How many minutes are needed to plate out 18.00 g of Ni from molten NiCl₂ using 6.93 A current? minutes are needed.arrow_forward
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