Calculate the number of moles of h2o removed and the moles of anhydrous cucl2 remaining in the crucible?

6.The moles of water can be gotten by dividing the mass of water in step 5 by the molecular mass of water(18.01528 g/mol).

7 The moles of the dried copper salt can be calculated  by dividing he mass of dried salt in step 4 by the molecular mass of CuCl2 (134.4620 g/mol).

Look below for further explanation

Explanation:

Assumption:The  lab experiment involved heating copper (II) chloride dihydrate in a crucible to remove the water.(hydrate)  

1. weigh and record the mass of  an empty crucible (tare wt).  

2.Add the copper hydrate salt, and reweigh (total  wt). The mass of the added hydrate salt can be derived by subtracting the tare wt from the total weight wt (= net wt of the hydrate).  

3.The next is to heat the crucible at some temperature above 100 C until the mass of the crucible plus dried salt is known to be constant (cool the crucible in a dessicator).  

4.The mass of the dried salt is obtained by subtracting the tare wt from the mass of the crucible plus dried salt. (mass of dried salt)

5.The mass of water is calculated by subtracting the mass of the dried salt from the mass of the hydrate salt.(in step 2)  

6.The moles of water can be gotten by dividing the mass of water in step 5 by the molecular mass of water(18.01528 g/mol).

7 The moles of the dried copper salt can be calculated  by dividing he mass of dried salt in step 4 by the molecular mass of CuCl2 (134.4620 g/mol).

what is the volume occupied by 40 grams of argon gas (ar) at standard conditions? what volume, in liters, is occupied by 1.5 x 1023 

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