(D)neither I nor II.S00mL of hydrogen at STP. How many mL of oxygen wouldAn electrolysis of water producesbe produced at STP?O2(g) + 2H2(g)2H20(I)(A)50 mL(B) 100 mL(C) 200 mL(D) It is impossible to tell without additional information.Open end1ti connected

Using given information one possible way to calculate the volume is as follows,The mass of water is…

Answered: (D)neither I nor II. S00 mL of hydrogen…

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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A current of 7.83×104 A is passed through an electrolysis cell containing molten KCI for 20.7 days. (a) How many grams of potassium are produced? 6.0 Submit Answer g (b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? L
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2 attempts left Be sure to answer all parts. To improve conductivity in the electroplating of automobile bumpers, a thin coating of copper separates the steel from a heavy coating of chromium. (a) What mass of Cu is deposited on an automobile trim piece if plating continues for 1.25 h at a current of 7.6 A? (b) If the area of the trim piece is 50.0 cm2, what is the thickness of the Cu coating?(d of Cu = 8.95 g/cm3)
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Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag ℰ° = +0.80 V Fe2+ + 2 e− → Fe ℰ° = −0.44 V (a) Determine the overall cell reaction and calculate ℰ ° cell . (b) Calculate ΔG° and K for the cell reaction at 25°C. (c) Calculate ℰcell at 25°C when [Ag+ ] = 1.0 ✕ 10−4 M and [Fe2+ ] = 1.0 ✕ 10−2 M.
In the electrolysis of water, how long will it take to produce 1.000 × 102 L of H2 at STP (273 K and 1.00 bar) using an electrolytic cell through which a current of 58.00 mA flows? Answer in yr
During electrorefining of Cu from CUSO4, how much time (in hours) is needed to produce 250 g Cu on the cathode if the current is kept at 11 A?
How many grams of A will be deposited on a cathode in 2.53 h by a current of 2.64 A? A ³+ + 3e- A(s) (MW of A is 51.21 g) Significant figures are not taken into account. 5.53 8.51 4.25
21.29 Consider the following voltaic cell: Voltmeter Fe Ni Salt bridge 1'M Fe2+ (a) In which direction do electrons flow in the external circuit? (b) In which half-cell does oxidation occur? (c) In which half-cell do electrons enter the cell? (d) At which electrode are electrons consumed? (e) Which electrode is negatively charged? (f) Which electrode decreases in mass during cell operation? (g) Suggest a solứtion for the cathode electrolyte. (h) Suggest a pair of ions for the salt bridge. (i) For which electrode could you use an inactive material? (i) In which direction do anions within the salt bridge move to maintain charge neutrality? (k) Write balanced half-reactions and an overall cell reaction.
A current of 8.86×104 A is passed through an electrolysis cell containing molten KCl for 12.7 days.(a) How many grams of potassium are produced? _________g(b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? _________L
Consider the electrolysis of molten calcium chloride with inert platinum electrodes. The following experimental observations were noted: • Bubbles of pale green chlorine gas are produced at one electrode, Shiny grey molten metallic calcium is produced at the other electrode. Ca2+( ()/Ca(s) E° =-2.84 V Cl2(g)/Cl-(e) E° = 1.36 V Explain what is happening. Your answer should include the following: • The redox processes happening at each electrode. Justify your choice of oxidation and reduction reactions using oxidation numbers and electron transfer. • Movement of the different identified charges. Relating all the observations to the species concerned. Balanced half and full equations. Discussion, with reasons, why this reaction is not spontaneous.

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(D)neither I nor II. S00 mL of hydrogen at STP. How many mL of oxygen would An electrolysis of water produces be produced at STP? O2(g) + 2H2(g) 2H20(I) (A)50 mL (B) 100 mL (C) 200 mL (D) It is impossible to tell without additional information. Open end 1ti connected