Chemistry

How many moles of electrons are required to produce 23.8 g Cu from a CuSO4 solution?

  1. 👍
  2. 👎
  3. 👁
  1. 96,485 coulombs are required to produce 1/2 mole Cu(63.546g/2); therefore, x coulombs are required to produce 23.8 g Cu. There are 6.022 x 10^23 electrons in 96,485 coulombs.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Calculate the volume of 1.0 M CuSO4 stock solution you should use to make 100 mL of a 0.010 m CuSO4 solution.

  2. chemistry

    How many grams of CuSO4 . 5H2O are needed to prepare 100ml of a 0.10M solution? Remember to change the given volume to liters and take the moles and convert them to grams via the molar mass to get grams of CuSO4 . 5H2O

  3. Chem 11

    So I did a lab determining the chemical formula of a hydrate. I really just need somebody to check this over for me. We had to find the molecular formula of a hydrate of copper (2) sulphate, CuSO4 .xH2O. My observation table looks

  4. Chemistry

    Iron metal reacts with oxygen gas to produce iron(III) oxide. If you have 12.0 moles of iron, for complete reaction you need: (HINT you need the balanced chemical reaction!) A) 9.0 moles of O2 and produce 3.0 moles of Fe2O3 B) 9.0

  1. chemistry

    A is a solution of trioxonitrate(v) acid, HNO3, of unknown concentration. B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution. 25cm3 portions solution B required an average of 24.00cm3 of solution A for

  2. Chemistry

    A is a solution of trioxonitrate (v)acid, HNO3 of unknown concentration.B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution. 25 cm3 portion solution B required an average of 24.00cm3 of solution A for

  3. Chemistry

    Given the balanced equation representing a reaction : 2Fe+ 3Cu^2+ --> 2Fe^3+ +3Cu When the iron atoms lose six moles of electrons, how many moles of electrons are gained by the copper ions? (1) 12 moles (2) 2 moles (3) 3 moles (4)

  4. chemistry

    How many grams of copper is deposited from an aqueous solution of copper sulfate, (CuSO4(aq)), by passing one mole of electrons into a copper plating cell? A. 254 g B. 127 g C. 63.5 g D. 42.3 g E. 31.8 g

  1. Chemistry

    The equation is: CuSO4(s) + Zn(s) -> Cu(s) + ZnSO4(aq) 3.22 g of powdered zinc is added to 200ml of 0.5M copper sulfate solution. What mass of copper is deposited? Hi guys. I am confused about the stoichmetry question. Q: The

  2. chemistry

    A chemist dissolves 0.097 g of CuSO4 ยท 5 H2O in water and dilutes the solution to the mark in a 500-mL volumetric flask. A 13.6-mL sample of this solution is then transferred to a second 500-mL volumetric flask and diluted. What

  3. Chemistry

    An aqueous solution is 8.50% ammonium chloride, NH4Cl, by mass. The density of the solution is 1.024g/mL. Calculate the molality, mole fraction, and molarity of NH4Cl in the solution. I know the formulas needed but I'm not sure

  4. Chemistry

    1. You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample

You can view more similar questions or ask a new question.