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.

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

0.88m hope i am correct : )