An aqueous solution of iron(II) sulfate (FeSO4) is prepared by dissolving 2.75 g in sufficient deionized water to form a 150.00 mL solution. Calculate the molarity of the solution.

The molarity of iron(II) sulfate solution is 0.724 M

Explanation:

To calculate the molarity of solution, we use the equation:

We are given:

Given mass of iron(II) sulfate = 2.75 g

Molar mass of iron(II) sulfate = 152 g/mol

Volume of solution = 150.0 mL

Putting values in above equation, we get:

Hence, the molarity of iron(II) sulfate solution is 0.724 M

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question: ray weighs 100 kilograms, his wrestling partner, bobby, weighs 50 kilograms. if ray moves at 4 m s , how fast will bobby have to run at him to apply an equal amount of kinetic energy?

answer: 8 m/s he needs to run twice as fast to keep up so he has some work to do

explanation:   if the mass has units of kilograms and the velocity of meters per second, the kinetic energy has units of kilograms-meters squared per second squared.

question answered by

(jacemorris04)