
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Transcribed Image Text:(d) How many grams of Ag would be deposited by supplying an electric current of 0.50 A for 30 min?
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- How many seconds are required to deposit 0.252 grams of tin metal from a solution that contains Sn* ions, if a current of 0.899 A is applied.arrow_forwardA current of 3.73 A is passed through a Cr(NO,), solution. How long, in hours, would this current have to be applied to plate out 6.90 g of chromium? time required:arrow_forwardHow many grams of zinc metal will be deposited from a solution that contains Zn^2+ ions if a current of 1.08 A is applied for 55.8 minutes.arrow_forward
- How many hours will it take to plate out all the copper in 250 ml of a 0.250 M Cu+ solution using a current of 0.650A?arrow_forwardThe answer is supposed to be in gramsarrow_forwardAn object with a surface area of 24.1 cm224.1 cm2 is to be plated with nickel. A current of 7.93 A7.93 A is applied to a solution containing nickel in the +2+2 oxidation state. Calculate the time required to coat the object with an even layer of nickel that is 9.71×10−3 cm9.71×10−3 cm thick. The density of nickel is 8.91 g/cm3.arrow_forward
- Electrosis... A current of 0.650 A deposits 0.413 g of a certain metal in 55.0 minutes. Calculate the atomic mass (molar mass) of the metal if n = 5 e− transferred per mole of metal. 92.9 31.0 183.9 50.9 114.8arrow_forwardI need hand written solution onlyarrow_forwardA current of 0.44A is passed through a solution of ruthenium nitrate causing reduction of the metal ion to the metal. After 25.0 minutes, 0.345g of Ru has been deposited. What is the charge on the ruthenium ion, Run+? What is the formula for ruthenium?arrow_forward
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