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2.3824g of anhydrous cuso4 were exposed to moist air for an extended period of time. Assuming that the hydrated salt formed is saturated with water to a limit consistent with the stoichiometric formula cuso4 5h2o, calculate the weight of the hydrated sample formed

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Nestor RutherfordLv2
17 Dec 2019
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Related questions

A 0.755-g sample of hydrated copper(II) sulfate, , was heated carefully until it had changed completely to anhydrous copper(II) sulfate (CuSO4) with a mass of 0.483 g. Determine the value of x. [This number is called the number of waters of hydration of copper(II) sulfate. It specifies the number of water molecules per formula unit of CuSO4 in the hydrated crystal.]

1.A hydrated form of copper sulfate (CuSO4·x H2O) is heated to drive off all the water. If we start with 9.19 g of hydrated salt and have 5.87 g of anhydrous CuSO4 after heating, find the number of water molecules associated with each CuSO4 formula unit.

2.Iron(II) Sulfate forms a blue-green hydrate with the formula FeSO4 ·n H2O(s). If this hydrate is heated to a high enough temperature, H2O(g) can be driven off, leaving the dirty yellow anhydrous salt FeSO4(s). A 18.300-g sample of the hydrate was heated to 300 °C. The resulting FeSO4(s) had a mass of 9.9993 g. Calculate the value of n in FeSO4 ·n H2O(s).

3.The combustion of ethane (C2H6) produces carbon dioxide and steam:

2C2H6 (G)+7O2(G)------->4CO2 (G)+6H2O (G)

How many moles of CO2 are produced when 5.15 mol of ethane are burned in an excess of oxygen?

--------MOLS?


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