Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Calculate the number of grams of aluminum produced in one hour by the
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- The electrolysis of AℓCℓ3 at high temperature produces aluminium metal. If a constant electrical current of 10.00 × 103?? flows for exactly one hour, calculate the number of aluminium atoms present in the metal produced during this time.arrow_forwardHow many milligrams of hydrogen can be produced by the electrolysis of water with a current of 0.308 A running for 5.00 min?arrow_forwardIn the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by electrolyzing brine, essentially an aqueous solution of sodium chloride. Suppose a current of 350. A is passed through an aqueous solution of NaCl for 54.0 seconds. Calculate the mass of pure chlorine produced. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol. 0 x10 0.0 μ 0|0 8 Śarrow_forward
- In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 2.35 amperes flowing for 140 minutes?arrow_forwardWhat volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of 2.69 A in 14.4 min?arrow_forwardWrite a balanced chemical equation (including states of matter) for an electrochemical cell that has a copper cathode immersed in a solution of Cu2+ ions, and a lead anode immersed in a solution of Pb2+ ions.arrow_forward
- Aluminum is produced commercially by the electrolysis of Al203 in the presence of a molten salt. If a plant has a continuous capacity of 1.09 million A, what mass of aluminum can be produced in 3.00 h? Mass = 5.94x10^5arrow_forwardIdentify those elements that can be prepared by electrolysisof their aqueous salts: strontium, gold, tin, chlorine.arrow_forwardHow many grams of iron may be formed by the passage of 6,931 C through an electrolytic cell that contains an aqueous ferrous (Fe(II)) salt.arrow_forward
- Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode reaction is below. 2 Cl −(aq) → Cl2(g) + 2 e− How long (in s) will it take to produce 1.09 kg of chlorine if the current is 6.00 102 A?arrow_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_forwardGold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCl4; it deposits on the cathode. Calculate the time it takes to deposit 0.34 gram of gold, passing a current of 0.10 amperes. (1 faraday = 96,485 coulombs)arrow_forward
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