AP Chemistry
1.3 Elemental Composition of Pure Substances
1.1 Moles and Molar Mass
A student heats a \(5.00 \text{ g}\) sample of hydrated copper(II) sulfate in a crucible according to the equation below.
\[ \text{CuSO}_4\cdot 5\text{H}_2\text{O}(s) \rightarrow \text{CuSO}_4(s) + 5\text{ H}_2\text{O}(g) \]
The molar mass of \(\text{CuSO}_4\cdot 5\text{H}_2\text{O}\) is \(250 \text{ g/mol}\), the molar mass of anhydrous \(\text{CuSO}_4\) is \(160 \text{ g/mol}\), and the molar mass of \(\text{H}_2\text{O}\) is \(18.0 \text{ g/mol}\). Assuming all water of hydration is completely driven off, what mass of \(\text{H}_2\text{O}(g)\) is released during the experiment?
\[ \text{CuSO}_4\cdot 5\text{H}_2\text{O}(s) \rightarrow \text{CuSO}_4(s) + 5\text{ H}_2\text{O}(g) \]
The molar mass of \(\text{CuSO}_4\cdot 5\text{H}_2\text{O}\) is \(250 \text{ g/mol}\), the molar mass of anhydrous \(\text{CuSO}_4\) is \(160 \text{ g/mol}\), and the molar mass of \(\text{H}_2\text{O}\) is \(18.0 \text{ g/mol}\). Assuming all water of hydration is completely driven off, what mass of \(\text{H}_2\text{O}(g)\) is released during the experiment?
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