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A chemist adds 370.0mL of a 2.25 M iron(III) bromide (FeBr3) solution to a reaction flask.

Calculate the mass in kilograms of iron(III) bromide the chemist has added to the flask.

Be sure your answer has the correct number of significant digits.

Respuesta :

Answer:

The mass of iron(III) bromide is 0.246 kg

Explanation:

Step 1: Data given

Volume of a FeBr3 solution = 370.00 mL = 0.370 L

Molarity of the FeBr3 solution = 2.25 M

Molar mass FeBr3 = 295.56 g/mol

Step 2: Calculate moles FeBr3

Moles FeBr3 = molarity FeBr3 solution * volume

Moles FeBr3 = 2.25 M * 0.370 M

Moles FeBr3 = 0.8325 moles

Step 3: Calculate mass FeBr3

Mass FeBr3 = moles FeBr3 * molar mass FeBr3

Mass FeBr3 = 0.8325 moles * 295.56g/mol

Mass FeBr3 = 246 grams = 0.246 Kg

The mass of iron(III) bromide is 0.246 kg

Answer: 0.246kg

Explanation:

V=370mL=0.370L

Molarity=2.25M

n=cv

Mole of FeBr3= 0.370*2.25

mole= 0.834

Molar mass of FeBr3=295.56g/mol

Mole= mass/molar mass

Mass= mole *molar mass

Mass=0.834*295.56

Mass=246.05g

Convert to kg

0.246kg

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