science

How do you calculate 1 mole of CuSO4 × 5 H2O?

  1. 👍
  2. 👎
  3. 👁
  1. Its mass will be 63.5 + 32 + 4*16 + 5*18 grams. Add them up. That is the total of the atmomic mass numbers for all atoms in the hydrated molecule. The 5*18 accounts for the five water molecules. I used 32 for S (sulfur) and 63.5 for copper, 1 for H and 16 for O.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    given the reactant amounts specified in each chemical eguation, determine the limiting reactant in each case: a. HCL+NaOH->NaCl+H2O 2.0 mole of HCl 2.5 mole NaOH b. Zn+2HCl->ZnCl2+H2 2.5 mole Zn 6.o mole HCl c.

  2. Chemistry (please help me!)

    H2(g) + CO2(g) H20(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured: [H2]=0.20 M [CO2]=0.30 M

  3. Chem

    Solid urea, (NH2)2CO, burns to give CO2,N2, and liquid H2O. Its heat of combustion is -632.2 kJ/mol. Balance the equation for combustion of urea, and calculate the heat generated per mole of H2O formed. (Enter in kJ.)

  4. 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

  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

    A mixture of CuSO4 and CuSO4·5 H2O has a mass of 1.235 g. After heating to drive off all the water, the mass is only 0.830 g. What is the mass percent of CuSO4·5 H2O in the mixture?

  3. Chemistry

    A)How many moles of O2 are required for the complete combustion of 2.2 g of C3H8 to form CO2 and H2O? b)A 65.25 g sample of CuSO4•5H2O (M = 249.7) is dissolved in enough water to make 0.800 L of solution. What volume of this

  4. chem

    One mole of H2O(g) at 1.00 atm and 100.°C occupies a volume of 30.6 L. When one mole of H2O(g) is condensed to one mole of H2O(l) at 1.00 atm and 100.°C, 40.66 kJ of heat is released. If the density of H2O(l) at this temperature

  1. Chemistry

    A 1.547-g sample of blue copper(II) sulfate pentahydrate, CuSO4*5H2O, is heated. The white crystals of CuSO4 that are left behind have a mass of 0.989 g. How many moles of H2O were in the original sample?

  2. Chemistry

    i need help. Calculate the pH of a 0.24 M CoCl3 solution. The Ka value for Co(H2O)63+ is 1.0 10-5. how do u do these with like the Cl there? Responses Chemistry - DrBob222, Monday, February 16, 2009 at 12:35am Just ignore the

  3. chemistry

    Calculate the number of moles of H2O formed when 0.200 mole of Ba(OH)2 is treated with 0.500 mol of HClO3 according to the chemical reaction shown below. Ba(OH)2 + 2 HClO3 ----> Ba(ClO3)2 + 2 H2O

  4. Chemistry

    Anhydrous CuSO4 can be used to dry liquids in which it is insoluble. The CuSO4 is converted to CuSO4 x 5H20, which can be filtered off from the liquid. What is the minimum mass of anhydrous CuSO4 needed to remove 12.6 g H20 from a

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