(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

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Chapter18: Electrochemistry

Section: Chapter Questions

Problem 99E: What volume of F2 gas, at 25C and 1.00 atm, is produced when molten KF is electrolyzed by a current...

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Hydrogen gas is produced when water is electrolyzed. 2H2O(g)2H2(g)+O2(g) A balloonist wants to fill a balloon with hydrogen gas. How long must a current of 12.0 A be used in the electrolysis of water to fill the balloon to a volume of 10.00 L and a pressure of 0.924 atm at 22°C?
13.106 Hydrazine, N2H4 , has been proposed as the fuel in a fuel cell in which oxygen is the oxidizing agent. The reactions are N2H4(aq)+4OH-(aq)N2(g)+4H2O(l)+4eO2(g)+2H2O(l)+4e4OH-(aq) (a) Which reaction occurs at the anode and which at the cathode? (b) What is the net cell reaction? (C) If the cell is to produce 0.50 A of current for 50.0 h, what mass in grams of hydrazine must be present? (d) What mass in grams of O2 must be available to react with the mass of N2H4 determined in part (c)?
Consider the electrolysis of NiCl2 to Ni(s) and Cl2(g). (a) What is the minimum voltage required to carry out this reaction at standard conditions? (b) If a voltage of 3.0 V is actually used, and 10.00 kJ of energy are consumed, how many grams of Ni(s) are obtained? (1J=1volt-coulomb)
Consider the production of 100 kg of sodium metal using a current of 50,000 A, assuming a 100% yield.. (a) How long will it take to produce the 100 kg of sodium metal?. (b)VVhatv01ume of chlorine at 25 C and 1.00 atm forms?
What volume of F2 gas, at 25C and 1.00 atm, is produced when molten KF is electrolyzed by a current of 10.0 A for 2.00 h? What mass of potassium metal is produced? At which electrode does each reaction occur?
In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?
A lead storage battery delivers a current of 6.00 A for one hour and 22 minutes at a voltage of 12.0 V. (a) How many grams of lead are converted to PbSO4? (b) How much electrical energy is produced in kilowatt hours?
A current is passed through a solution of copper(II) sulfate long enough to deposit 14.5 g of copper. What volume of oxygen is also produced if the gas is measured at 24 °C and 0.958 atm of pressure?
In the electrolysis of a solution containing Ni2+(aq), metallic Ni(s) deposits on the cathode. Using a current of 0.150 A for 12.2 minutes, what mass of nickel will form?
Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)

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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