Chemistry

A student was isolating copper metal from a copper salt. If the student started with 1.255g of copper (II) sulfate how many grams of copper solid would you expect them to recover?

asked by Caroline
  1. 1.225 g CuSO4 x (atomic mass Cu/molar mass CuSO4) = ?

    In reality that CuSO4 probably was CuSO4.5H2O.

    posted by DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. chem

    A student determines the composition of a copper chloride compound. Tell whether each of the situations described below would cause the student’s experimental value for the percent of copper in the compound to be greater than
  2. College Chemistry 104

    Students are attempting to construct a battery in the laboratory that will light up a light bulb. Compare the following lists prepared by students and determine which student will not be able to successfully build a "battery" that
  3. Chemistry

    a student used a piece of copper with a mass of 2.85g and obtained 2.95g of copper at the end of the experiment, an apparent recovery of 104$. How could the student account for this result, since the best to expect is 100%.
  4. Chemistry - Science (Dr. Bob222)

    A student wanted to determine the amount of copper in a sample of copper ore. The student dissolved a 2.500 ± 0.001 g piece of copper ore in about 75 mL of nitric acid; then, a complexing agent was added. The student transferred
  5. College Gen.Chemistry

    A student wanted to determine the amount of copper in a sample of copper ore. The student dissolved a 2.500 ± 0.001 g piece of copper ore in about 75 mL of nitric acid; then, a complexing agent was added. The student transferred
  6. Chemistry

    is it easy to distinguish between between the different oxidation states of copper? why? -I answered yes because copper (I) is not as stable as copper (II), and there is a noticeable colour difference You synthesized copper (I)
  7. chem

    A greenish blue salt known to be composed of copper and chloride ions is dissolved in DI water. Aluminum metal is used to reduce the copper ions to metallic copper, which is collected, dried and weighed. If the origanal sample has
  8. CHEMESTRY

    a student heats 2.005 g of a copper bromide hydrate of unknown molecular formula, completely driving off the water of hydration, and notices that the weight drops to 0.998g. Upon reduction with excess aluminum metal, the copper
  9. Chemistry

    A student begins with 9.7 mL of a 0.26 M Cu(NO3)2 solution and performs copper cycle lab. She recovers 0.075 grams of copper metal. A) What is the Theoretical Yield B) What is the Actual Yield C) What is the Percent Yield
  10. Chemistry

    A student used 5.06g of copper sulphate pentahydrate and salicyclic acid in the performance of the experiment. The student recovered 3.094g of salicyclic acid and 2.146g of copper sulphate pentahydrate. What is wrong with the

More Similar Questions