If you had dehydrated 1.00g of the hydrate CaCl2 ∙6H2O how many grams of anhydrous CaCl2 would you expect to be produced? Show calculations.

I really am having a hard time with this question. I don't know where to start and how to perform it.

There's the long way, a shorter way, and a short cut that isn't taught in schools anymore.

Long way.
mols CaCl2.6H2O = grams/molar mass = ?
mols CaCl2 = mols CaCl2.6H2O since there is 1 mol CaCl2 in 1 mol CaCl2.6H2O
Finally, g CaCl2 = mols CaCl2 x molar mass CaCl2.

shorter way.
% CaCl2 in CaCl2.6H2O = (molar mass CaCl2/molar mass CaCl2.6H2O)*100 = ?
Then 1 g*(%CaCl2/100) = ?g CaCl2.

Shortcut way not taught now.
1 g x (molar mass CaCl2/molar mass CaCl2.6H2O = ?g CaCl2.

Well, fret not my friend! Let's dive into this question together with a sprinkling of humor, shall we?

To calculate the grams of anhydrous CaCl2 produced, we need to consider the molar masses of both the hydrate and anhydrous compound.

First, let's tackle the hydrate CaCl2 ∙ 6H2O. The molar mass of one molecule of CaCl2 is approximately 110.98 g/mol. The molar mass of 6 water molecules (H2O) is about 6.02 g/mol.

So, for one mole of the hydrate CaCl2 ∙ 6H2O, the total molar mass would be:
(1 mole x 110.98 g/mol) + (6 moles x 18.02 g/mol) = 219.92 g/mol.

Since you have 1.00g of the hydrate, you can set up a simple ratio:
1.00 g / 219.92 g/mol = x g / 1 mol.

Solving for x gives:
x = (1.00 g)(1 mol) / 219.92 g/mol ≈ 0.0045 mol.

Now we can move on to finding the grams of anhydrous CaCl2 produced. The molar mass of anhydrous CaCl2 is approximately 110.98 g/mol.

Using the stoichiometry of the equation, we know that 1 mole of the hydrate (CaCl2 ∙ 6H2O) yields 1 mole of anhydrous CaCl2.

Therefore, the grams of anhydrous CaCl2 produced can be calculated as:
0.0045 mol x 110.98 g/mol ≈ 0.50 g.

So, when you dehydrate 1.00 g of the hydrate CaCl2 ∙ 6H2O, you would expect to produce approximately 0.50 g of anhydrous CaCl2. Et voila!

Don't worry, I'm here to help! To solve this problem, we need to use the concept of the molar mass and apply stoichiometry. Here's a step-by-step guide on how to approach this question:

1. Determine the molar mass of the hydrated compound (CaCl2 ∙ 6H2O). To do this, we add up the individual molar masses of each element present in the compound. The molar mass of calcium chloride (CaCl2) is approximately 110.98 g/mol, and the molar mass of water (H2O) is approximately 18.015 g/mol. Adding these values together gives us:

Molar mass of CaCl2 ∙ 6H2O = (110.98 g/mol) + (6 × 18.015 g/mol)

2. Calculate the molar mass of the anhydrous compound (CaCl2). The molar mass of calcium chloride (CaCl2) is the same as we determined earlier.

3. Calculate the molar mass of the water present in the hydrated compound. Since the molecular formula of water in the hydrated compound is 6H2O, the molar mass of water is 6 times the molar mass of H2O.

Molar mass of water in CaCl2 ∙ 6H2O = 6 × 18.015 g/mol

4. Determine the mass of water in the hydrated compound. Since the hydrated compound has a mass of 1.00g, all of it is due to the combined mass of the anhydrous compound and water. Subtracting the molar mass of the anhydrous compound from the molar mass of the hydrated compound gives the molar mass of water.

Mass of water = Molar mass of CaCl2 ∙ 6H2O - Molar mass of CaCl2

5. Calculate the number of moles of water in the hydrated compound. The number of moles can be found by dividing the mass of water by its molar mass.

Number of moles of water = Mass of water / Molar mass of water

6. Use the stoichiometry of the chemical equation to determine the number of moles of anhydrous CaCl2 produced. Recall that the ratio between anhydrous CaCl2 and water in the hydrate is 1:6 (from the formula CaCl2 ∙ 6H2O).

Number of moles of CaCl2 = Number of moles of water / 6

7. Finally, calculate the mass of anhydrous CaCl2 using the number of moles of CaCl2 and the molar mass of CaCl2.

Mass of anhydrous CaCl2 = Number of moles of CaCl2 × Molar mass of CaCl2

By following these steps and substituting the given values into the appropriate equations, you will be able to calculate the mass of anhydrous CaCl2 expected to be produced.