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2 years ago

Consider the hydrate FeSO4 • 7H2O.

2 answers:

7 0

The molar mass of the hydrate is 278.06
The molar mass of the anhydrous salt is 151.92
The molar mass of water in the hydrate is 126.14

mr_godi [17]2 years ago

7 0

Answer: The molar mass of the hydrate $FeSO_4$ . $7H_2O$ is 278g. The molar mass of the anhydrous salt $FeSO_4$ is 152 g. The molar mass of the water in the hydrate is $H_2O$ is 126g.

Explanation: Molar mass of Fe = 56 g

Molar mass of of S = 32 g

Molar mass of O = 16 g

Molar mass of H = 1 g

Molar mass of $FeSO_4$ • $7H_2O$ = $1\times \text{molar mass of Fe}+1\times \text{molar mass of S}+11\times \text{molar mass of O}+14\times \text{molar mass of H}$

Molar mass of $FeSO_4$ • $7H_2O$ = $1\times 56+1\times 32+11\times 16+14\times 1=278g$

Molar mass of $FeSO_4=1\times \text{molar mass of Fe}+1\times \text{molar mass of S}+4\times \text{molar mass of O}$

Molar mass of $FeSO_4=1\times 56+1\times 32+4\times 16=152g$

Molar mass of $7H_2O=14\times \text{molar mass of H}+7\times \text{molar mass of O}$

Molar mass of $7H_2O=14\times 1+7\times 16=126g$

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Acetone (C₃H₆O) has a boiling point of 56.5 °C. How many grams of the acetone vapor would occupy the 250 mL Erlenmeyer flask at 57 °C and 730 mmHg?

Step 1: Given data

Temperature (T): 57°C

Pressure (P): 730 mmHg

Volume (V): 250 mL

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We will use the following expression.

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We will use the ideal gas equation.

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