posted by .

if you heat 15.00g of the hydrate CaSO4*2H20, and drive off the water, what is the weight of the anhydrous salt remaining?

How do I go about solving this?

  • chemistry -

    Just make it a regular stoichiometry problem.
    CaSO4*2H2O ==> CaSO4 + 2H2O

  • chemistry -

    so then would i find the gfm of the CaSO4?
    and get 136.2 as my answer?

  • chemistry -

    Do you really believe you can start with 15.00 g CaSO4.2H2O, lose the water, and end up with more than 15.00 g? Not likely. It MUST be less than 15.00 grams CaSO4.
    CaSO4.2H2O ==> CaSO4 + 2H2O

    moles CaSO4.2H2O = 15.00 g x (1 mole CaSO4.2H2O/172.172) = 0.08712 moles.

    moles CaSO4 = same.
    grams CaSO4 = moles CaSO4 x molar mass CaSO4 = ??

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    What percent by mass does the water constitute in Na2SO4*10H2O?
  2. chemistry 11

    Hi, I am stuck on a couple questions in chemistry 11. The questions are 1. Calculate the number of moles of the anhydrous salt left behind 2. Calculate the number of moles of water removed by heat from your sample of hydrate. 3. Calculate …
  3. Chemistry

    Below are the formulas of some hydrates. what is the mole ratio of salt to water?
  4. chemestry

    1.0000 g of hydrate of stannic chloride with unknown formula is heated to 100C (celsius) for 30 minutes. The remaining anhydrous salt weighted 0.7836g. What is the formula of this hydrate?
  5. Chemistry

    A 5 gram sample of a hydrate of BaCL2 was heated, and only 4.3g of the anhydrous salt remained. What percentage of water was in the hydrate?
  6. Chemistry

    A 2.914 gram sample of gypsum, a hydrated salt of calcium sulfat, CaSO4, is heated at a temperature greater than 170 degrees Celcius in a crucible until a constant mass is reached. The mass of the anhydrous CaSO4 salt is 2.304 grams. …
  7. chemistry

    a 5.00g sample of a hydrate of barium chloride was heated, and only 4.30g of the anhydrous salt remained. what is the formula of the hydrate?
  8. Chemistry

    A solid sample of a hydrate salt, NaNO3xH2O, was heated gently to drive off all the water of crystallization. Starting with a mass of 7.494g of NaNO3xH2O, a mass of 5.263g of the anhydrous salt, NaNO3 was obtained. Determine the value …

    is this right? 5. After heating the crucible is set on the lab bench where it is contaminated with the cleaning oil used to clean the lab bench but before its mass is measured. The analysis continues where the mass of the anhydrous
  10. Chemistry

    7. A student conducts an experiment on a different hydrate. The empty crucible is heated to a constant mass of 24.330. A sample of the unidentified hydrate is placed in the crucible, and the total mass is 31.571 g. The crucible and …

More Similar Questions