A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours. Calculate the mass (in grams) of cadmium metal deposited. [Enter only numbers in the blank.]

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  1. Chemistry

    A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours. Calculate the mass (in grams) of cadmium metal deposited. [Enter only numbers in the blank.]

  2. Easy chemistry

    Which statement correctly identifies how a lead-storage battery in a car works? A. The battery acts as a galvanic cell as it provides current to the radio. B. The battery acts as a galvanic cell as it is recharged by the alternator. C. The battery acts as

  3. Chemistry

    How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO4 for a period of 19.0 min?

  4. chemistry- electrochemical cell

    What makes this an oxidation-reaction? 3Ag2S+2Al(s) -> Al2S3+6 Ag(s)? Write the half-reactions showing the oxidation and reduction reactions. Identify which is the oxidation reaction and which is the reduction reason. What is oxidized in the reaction? What

  5. chemistry

    Current is applied to a molten mixture of CuF, ZnCl2, and AlBr3. What is produced at the cathode? a)F2 b)Al c)Cu d)Zn e)Cl2 f)Br2 What is produced at the anode? Same options as above.

  6. Chemistry

    Elemental calcium is produced by the electrolysis of molten CaCl2. a) What mass of calcium can be produced by this process if a current of 7.5 * 10^3 A is applied for 48h? Assume that the electrolytic cell is 68% efficient. b) What is he minimum voltage

  7. Physics

    The internal resistance of a dry cell increases gradually with age, even though the cell is not used. The emf, however, remains fairly constant at 1.5 V. Dry cells must be tested for age at the time of purchase by connecting an ammeter directly across the

  8. Chemistry

    Which statement correctly identifies how a lead-storage battery in a car works? A. The battery acts as a galvanic cell as it provides current to the radio. B. The battery acts as a galvanic cell as it is recharged by the alternator. C. The battery acts as

  9. Chem

    How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu2+ ions to produce 4.00 moles of copper metal?

  10. ap

    The reaction 2Na+ + 2Cl− ! 2Na + Cl2 is indicative of ? cell; the sign of the anode is ? ; and ? forms at the cathode. 1. an electrolytic; negative; Na+ 2. a voltaic; positive; Na 3. an electrolytic; positive; Na 4. an electrolytic; positive; Cl2 5. a

  11. Chemistry

    A zinc-copper battery is constructed as follows at 25°C. Zn|Zn^2+ (0.15 M)||Cu2+(3.00 M)|Cu The mass of each electrode is 200. g. a) Calculate the cell potential when this battery is first connected. - i got this to be 1.14V b.) Calculate the cell

  12. Chemistry

    1. A student wishes to set up an electrolytic cell to plate copper onto a belt buckle. Predict the length of time it will take to plate out 2.5g of copper from a copper (II) nitrate solution using 2.5A current. At which electrode should the buckle be

  13. Chemistry

    Consider two cells, the first with Al and Ag electrodes, and the second with Zn and Ni electrodes, each in appropriate 1.00M solutions of their ions. If 2.10g of metal is plated in the voltaic cell, how much metal is plated in the electrolytic cell?

  14. Chemistry

    How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu2+ ions to produce 3.00 moles of copper metal?

  15. Chemistry

    1. Which of the following metals is oxidized by calcium ions? *potassium zinc iron lead 2. The first electrochemical cell was invented by ____. Michael Faraday *Alessandro Volta James Maxwell Benjamin Franklin 3. Why can't a lead storage battery be

  16. Chemistry: Please check answers

    12. What balances charges that may build up as reduction and oxidation occur in a voltaic cell? *the salt bridge one of the half-cells the electrolyte solutions the moving electrons 13. What is the electrode in the center of the most common dry cell made

  17. Chemistry

    A current is passed through three electrolytic cells containing silver trixonitrate(5),coppe(2)tetraoxonitrate(6) and brine respectively.if 12.7g of copper are deposited in the second electrolytic cell.calculate(a)the mass of silver deposited in d first

  18. NEED HELP! CHEMISTRY

    Three electrolytic cells containing solutions of CuNO3, Sn(NO3)2, and Fe(NO3)3, respectively, are connected in series. A current of 2.2 A is passed through the cells until 3.10 g of copper has been deposited in the cell. (a) What masses of tin and iron are

  19. Chemistry

    A student wishes to set up an electrolytic cell to plate copper onto a belt buckle. Predict the length of time it will take to plate out 2.5g of copper from a copper (II) nitrate solution using a 2.5-A current. At which electrode should the buckle be

  20. chemistry

    During the electrolysis of molten aluminum chloride in an electrolytic cell, 5.40 g of aluminum is produced at the cathode. Predict the mass of chlorine produced at the anode.

  21. Chemistry

    Little confusing!! I need help PLZ!!! Two half cells in a galvanic cell consist of one iron (Fe(s)) electrode in a solution of iron (II) sulphate (FeSO4(aq)) and a silver (Ag(s)) electrode in a silver nitrate solution. a. Assume the cell is operating as a

  22. Physical Chemistry

    Three electrolytic cells containing solutions of CuNO3, Sn(NO3)2, and Fe(NO3)3, respectively, are connected in series. A current of 2.2 A is passed through the cells until 3.10 g of copper has been deposited in the cell. (a) What masses of tin and iron are

  23. Solar Energy Help ASAP

    The current density of an ideal p-n junction under illumination can be described by: J(V)=Jph−J0(eqVkT−1) where Jph is the photo-current density, J0 the saturation-current density, q the elementary charge, V the voltage, k the Boltzmann's constant, and

  24. Chem -plz check work

    so i've worked on this some more, now I am asking if someone will plz check my work 2 half cells in a galvanic cell consist of one iron Fe(s) electorde in a solution of iron (II) sulphate FeSO4(aq)and a silver Ag(s) electrode in a silver nitrate solution,

  25. CHEMISTRY

    Chromium plating is done using a dichromate solution. How long would it take to plate 1.0x10-2mm thick onto a car bumper with surface area 0.25m^2 in a 25.0 Amp electrolytic cell? (density of chromium is 7.19g/cm^3)

  26. chemistry

    An electrolytic cell transferred 0.10 mol of electrons when a constant current of 2.0 A was applied. How many hours did this take? A. 4800h B. 80h C. 1.3h D. 0.75h E. 0.012h

  27. chemistry

    How many minutes does it take to form 10.0L of O2 Measured at 99.8kpa and 28 C from water if a current of 1.3A passes through the electrolytic cell? what mass of h2 forms?

  28. Chemistry

    Aluminum is produced by the electrolysis of aluminum oxide (Al2O3, bauxite ore) dissolved in molten cryolyte (Na2AlF6). Calculate the mass of aluminum that can be produced in one day in an electrolytic cell operating continuously at 1.0 x 105 amps. The

  29. Chemistry

    How many hours will it take to produce 78.0 g of Al metal by the reduction of Al3+ in an electrolytic cell with a current of 2.00 Amperes? [Enter only a number for your answer.]

  30. Chemistry

    Determine the mass of chlorine produced when 200A of current flows for 24 hours through a cell of molten NaCl.

  31. Physics

    When a nerve cell depolarizes, charge is transferred across the cell membrane, changing the potential difference. For a typical nerve cell, 9.0 pC of charge flows in a time of 0.50ms. What is the average current(Value and units)?

  32. college chemistry

    A zinc-copper battery is constructed as follows: Zn | Zn+2(0.10 M) || Cu+2 (2.50 M)| Cu The mass of each electrode is 200.0 g. Each half cell contains 1.00 liter of solution. a) Calculate the cell potential when this battery is first connected. b)

  33. Physics

    A cell of emf 2v and internal resistance of 1ohms passes a current through an external load of 9ohms.calculate the potential difference across the cell

  34. erectlo chemistry

    ADDIS ABABA UNIVERSITY ADDIS ABABA INSTITUTE OF TECHNOLOGY SCHOOL OF CHEMICAL AND BIO ENGINEERING Applied Electrochemistry WORKSHEET -1 1. Calculate the standard potential of each of the following cells. State which one(s), if any, will proceed

  35. chemistry

    If a current of 5.0 Amps is passed through the electrolytic cell for .5 hour, how should you calculate the number of grams of bromine produced?

  36. apchemistry

    Hi Please double check me: I had to state whether the process forms a voltaic or eletrolytic cell: YOu plug in your MP3 player to charge the nickel-cadmium battery (I said electrolytic)??? The radio plays in your car even though the engine is not running.

  37. Chemistry

    5. Explain the difference between a galvanic (voltaic) cell and an electrolytic cell. For a reaction in a galvanic cell, change in S is negative. Which of the following statements is true? Defend your answer. a."E"willncrease with an increase in

  38. chemistry

    Chromium is reduced from CrO4{2-} to Cr(OH)4- in an electrolytic cell. What mass of Cr(OH)4- is formed by passage of 4.50 A for a period of 8000 seconds?

  39. Chemistry

    calculate the quantity of electricity passed when 0.4A flows for 1hr 20minutes through an electrolytic cell. (a) 4800C (b) 3840C (c) 1920C (d) 32C?

  40. College Chemistry

    If current is passed in an electrolytic cell containing sodium nitrate, NaNO3, dissolved in water, what are the products at the anode and the cathode? If it's dissolved in water then it is: NaNO3 -> Na+ + NO3- right? So you have... Anode: NaNO3 -> Na+ + e-

  41. Chemistry

    In every electrolytic and galvanic (voltaic) cell the anode is that electrode (A) at which oxidation occurs. (B) which attracts cations. (C) at which electrons are supplied to the solution. (D) at which reduction occurs.

  42. chemistry

    Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 6.7×104 A flowing for a period of 23 h . Assume the electrolytic cell is 86 % efficient. What is the energy requirement for this electrolysis per mole of Li formed if the

  43. chemistry

    What is the difference between a galvanic cell and an electrolytic cell? A. A galvanic cell converts reduction reactions into an electrolytic cell, and an electrolytic cell converts oxidation reactions into a galvanic cell. B. A galvanic cell converts

  44. chemistry

    Observe the diagram of the electrolytic cell (A aqueous solution of molten salt with a power supply). The molten salt is lithium flouride. Write the half reaction occuring at the cathode, following the usual style guide and making sure to balance

  45. chem

    Explain, in terms of electrical energy, how the operation of a voltaic cell differs from the operation of an electrolytic cell used in the Hall process. Include both the voltaic cell and the electrolytic cell in your answer. Would this be correct: In a

  46. Chemistry

    Given cell Cd | CdCl2 (0.55M) || NaBrO3 (0.34M), NaBr (0.12M), pH=1.20 | Pt 1. How many electrons are transferred? 2. What is E° for the cell? 3. What is E for the cell?

  47. Chemistry

    What happens to the current flow with time in an electrolytic cell ? explain. thank for helping~

  48. Physics

    If 3.25x10-3 kg of gold is deposited onto the negative electrode of an electrolytic cell in a period of 2.78 hours, what is the current through this cell in amperes? Assume that the gold ions carry one elementary unit of charge

  49. Physics

    If 3.25x10-3 kg of gold is deposited onto the negative electrode of an electrolytic cell in a period of 2.78 hours, what is the current through this cell in amperes? Assume that the gold ions carry one elementary unit of charge

  50. Physics

    If 3.25x10-3 kg of gold is deposited onto the negative electrode of an electrolytic cell in a period of 2.78 hours, what is the current through this cell in amperes? Assume that the gold ions carry one elementary unit of charge

  51. Chemistry physics

    3.25x10-3 kg of gold is deposited onto the negative electrode of an electrolytic cell in a period of 2.78 hours, what is the current through this cell in amperes? Assume that the gold ions carry one elementary unit of charge

  52. Chemistry

    How many moles of electrons are involved in an electrolytic process if 3.07 amps are applied to the cell for 46.0 hours? The answer is 5.27, but I'm not sure how to get there. Please help!

  53. Chemistry again

    Two voltaic cells are to be joined so that one will run the other as an electrolytic cell. In the first cell, one half-cell has Au foil in 1.00M Au(NO3)3, and the other half-cell has a Cr bar in 1.00M Cr(NO3)3. In the second cell, one half-cell has a Co

  54. Chemistry

    A current of 2.34 A is delivered to an electrolytic cell for 85 minutes. How many grams of Au will be deposited from an aqueous solution of AuCl3?

  55. Chemistry

    A current of 2.34 A is delivered to an electrolytic cell for 85 minutes. How many grams of Au will be deposited from an aqueous solution of AuCl3?

  56. Electrolysis

    A current of 1.2A was passed through an electrolytic cell containing dilute Tetraoxosulphate(VI) for 40minutes. Calculate the volume of gas produced at s.t.p.

  57. Chemistry

    Elemental calcium is produced by the electrolysis of molen CaCl2. What mass of calcium can be produced by this process if a current of 8500 A is applied for 39 h? Assume that the electrolytic cell is 65% efficient. I found the mass to equal 1.6 x10^5g Ca,

  58. Chemistry

    Elemental calcium is produced by the electrolysis of molen CaCl2. What mass of calcium can be produced by this process if a current of 8500 A is applied for 39 h? Assume that the electrolytic cell is 65% efficient. I found the mass to equal 1.6 x10^5g Ca,

  59. chemistry

    Molten Al2O3 is reduced by electrolysis at low potentials and high currents. If 1.5 x 10^4 amperes of current is passed through molten Al2O3 for 8.0 hours, what mass of Al is produced? Assume 100% current efficiency? Mdep = ([1.5 x 10^ x 28800s ]/ 96500) x

  60. chemistry

    How many grams of copper will be deposited at the cathode of an electrolytic cell if a current of 680.0 mA is run through a 2.5 M solution of copper sulfate for 20.0 minutes?

  61. Physics

    Calculate the amount of copper deposited in a zinc/Copper electrode of electrolytic cell when 2.5A of electric current is passed in 10 minutes?

  62. Chemistry

    Consider the NiCd (nickle cadmium) cell found in rechargeable batteries. 1.)Which element is the cathode when the cell is recharging (being electrolytic)? 2.)How many cells must be present to produce 1.2 V 3.)Which element is the anode when the cell is

  63. Chemistiy

    Check if im right please. a. oxidation occurs at my anode ____ ** Voltaic Cell b. You can use standard reduction potential table to calculate how much voltage it takes to operate me____ **Both voltaic cell and electrolytic cell

  64. Chem 2

    Metallic Magnesium can be made from electrolysis of molten MgCl2. What mass of Mg is formed by passing a current of 4.55A through a molten MgCl2 for 3.50 days? Please Help!!

  65. Chemistry

    1. Distinguish between a conductor and electrolyte. 2. State Faraday's first law of electrolysis 3. What is an electrochemical cell 4. State five differences between an electrochemical cell and electrolytic cell.

  66. chemistry

    Dr Bob Could you check this please? Voltaic cell---cathode is positive, accepts electrons, reduced, anode is negative, gives up electrons and is oxidized Electrolytic cell------cathode is negative, accepts electrons and is reduced. Anode is positive,

  67. Algebra

    The electric current I in a circuit varies directly as the voltage V. When 21V are applied, the current is 4A. What is the current when 18 volts are applied

  68. Math

    The electric current I in a circuit varies directly as the voltage V. When 21V are applied, the current is 4A. What is the current when 18 volts are applied

  69. chem. stuff+5

    9. The reaction 2 H2O(l)>>>O2(g) + 2 H2(g) requires 2.06 V, but the reaction 2 H2O(l) + 2 Cl –(aq)>>> H2(g) + 2 OH –(aq) + Cl2(g) requires 2.19 V. If a 1.0 mol/L solution of aqueous NaCl is electrolyzed, what voltage should be applied to get O2(g), but

  70. Chemistry

    If a current of 3.00 A is applied to a cell containing a 400g copper anode, determine the final mass of the copper anode after the cell runs for 48.0h

  71. grade 12 chemisstry

    I have no idea what I'm doing here, please help. 2 half cells in a galvanic cell consist of one iron Fe(s) electorde in a solution of iron (II) sulphate FeSO4(aq)and a silver Ag(s) electrode in a silver nitrate solution, a)state the oxidation half

  72. CHEMISTRY

    Why can't we use water in electrolytic cell during producing aluminium ?

  73. Chemistry

    What's the difference between a galvanic and electrolytic cell when trying to find which half-rxn is the anode or the cathode? So like when you have two equations, depending on what kind of cell it's in, how can you tell which one is the anode and which

  74. Chemistry

    The molten lead obtained from the blast furnace contains 0.1% of silver dissolved as an impurity. The silver is removed by: -adding zinc to the mixture of molten lead and silver at 350'C and removing the mixture of molten zinc and silver that forms on top

  75. college chemistry

    predict the order of reduction and which of the following ions will reduce first at the cathode of an electrolytic cell: Ag^(+), Zn^(+2), IO3^(-)?

  76. science

    What energy changes occur in an electrochemical cell when electric current flows from it? This is what I put down but I am not sure if it is right... In a primary cell, chemical reactions use up some of the materials in the cell as electrons flow from it.

  77. Chemistry

    Why are molten metal chlorides used as electrolytes rather than using other molten salts? Thanks for ur helps alot.

  78. CHEMISTRY! Help?

    If 4.00 g of metal is plated in the voltaic cell (which contains Ag and Ni with the total potential of 2.98 V) , how much metal is plated in the electrolytic cell (contains Ag and Zn with the total of 1.98 V)? I have no idea how to do this! Help?

  79. chemistry

    If 4.00 g of metal is plated in the voltaic cell (which contains Ag and Ni with the total potential of 2.98 V) , how much metal is plated in the electrolytic cell (contains Ag and Zn with the total of 1.98 V)? I have no idea how to do this! Help?

  80. Chemistry

    If 4.00 g of metal is plated in the voltaic cell (which contains Ag and Ni with the total potential of 2.98 V) , how much metal is plated in the electrolytic cell (contains Ag and Zn with the total of 1.98 V)? I have no idea how to do this! Help?

  81. Gen Chem

    A current is passed through two cells connected in series. The half-reactions occurring at the cathode of each cell are TcO4-(aq) + 8 H+(aq) + 7 e- ===> Tc(s) + 4 H2O(l) and Cu2+(aq) + 2 e- ===> Cu(s). If 4.40 g of copper are deposited in the second cell,

  82. chemistry

    How many minutes are needed to plate out 29.00g Mg from molten MgCl2, using 2.70A of current?

  83. Chemistry

    How many hours are required for the deposition of 15.0 grams of Al from molten AlCl3 by a current of 15.0 amps?

  84. Neuroscience

    I'm struggling with the following question: The opening of chloride selective channels by a neurotransmitter X will drive membrane potential toward the chloride equilibrium potential. Assume that early during cell development, Cl is pumped into the cell

  85. chemistry

    consider the electrolysis of molten AlCl3 what must the current be in amps if you need to obtain 25.0 grams of aluminum in 5.00 min

  86. chemistry

    an electrolytic cell requires a salt bridge. true or false I say true

  87. ET3034TUx Solar Energy

    The current density of an ideal p-n junction under illumination can be described by: J(V)=Jph−J0(eqVkT−1) where Jph is the photo-current density, J0 the saturation-current density, q the elementary charge, V the voltage, k the Boltzmann's constant, and

  88. CHEMISTRY

    If 4.00 g of metal is plated in the voltaic cell (which contains Ag and Ni with the total potential of 2.98 V) , how much metal is plated in the electrolytic cell (contains Ag and Zn with the total of 1.98 V)?

  89. AP Chemistry

    A total charge of 96.5 kC is passed through an electrolytic cell. What mass of copper will be produced from a copper(II) chloride solution? Answer in units of g

  90. Chemistry

    Given that the battery produces a current of 2.5A that passes through molten zinc chloride for 3 minutes what charge would be dissipated through the electrolyte

  91. ap chemistry

    A total charge of 96.5 kC is passed through an electrolytic cell. What mass of silver metal will be produced from a silver nitrate solution? Answer in units of g

  92. Chemistry

    For the following battery: Cd(s) | CdCl2(aq) || Cl–(aq) | Cl2(l) | C(s) (a) Write the reduction half-reaction occuring at the C(s) electrode. (Include physical states of reactants and products.) C(s) electrode:? (c) Calculate the mass of Cl2 consumed if

  93. Physics

    There is current of 115 pA when a certain potential is applied across a certain resistor. When that same potential is applied across a resistor made of the identical material but 30 times longer, the current is 0.044 pA. Compare the effective diameters of

  94. Homework Help: Solar Energy Please HelpASAP

    d) In the up-convertor 1, two photons are converted into one photon with 100% conversion efficiency. If all photons with energy above that of the band gap of a-SiC:H are absorbed in the a-SiC:H layer, in which spectral range can the photons be up-converted

  95. chemistry

    Consider two cells, the first with Al and Ag electrodes, and the second with Zn and Ni electrodes, each in appropriate 1.00 M solutions of their ions. a) If connected as voltaic cells in series, which two metals are plated, and what is the total potential?

  96. Chemistry

    What are the signs of dH, dS, and dG for the following and please explain why? Also what does it mean by sublimation, and molten? 1. CO2(s) --> CO2(g) (Dry ice subliming) dH = ? dS = ? dG = ? 2. The electrolysis of molten NaCl(l). dH = ? dS = ? dG = ?

  97. Chemistry -please help!

    A zinc-copper battery is constructed as follows at 25°C. Zn|Zn^2+ (0.15 M)||Cu2+(3.00 M)|Cu The mass of each electrode is 200. g. a) Calculate the cell potential when this battery is first connected. - i got this to be 1.14V b.) Calculate the cell

  98. chemistry

    Consider two cells, the first with Al and Ag electrodes, and the second with Zn and Ni electrodes, each in appropriate 1.00 M solutions of their ions. a) If connected as voltaic cells in series, which two metals are plated, and what is the total potential?

  99. Chem

    What equation can I use to solve this kind of problem? A metal undergoes electrolytic reduction according to ne- + Mn+ ===> M. What current (in Ampères) must be provided to deposit the metal at a rate of 1.914 mol/hr if n = 3?

  100. Chemistry

    A current of 3.94 A is pass through a Pb(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 5.40 g of lead?

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