When 3.24 g of a nonelectrolyte solute is dissolved in water to make 955 mL of solution at 22 °C, the solution exerts an osmotic pressure of 973 torr. What is the molar concentration of the solution? concentration: M How many moles of solute are in the solution? moles of solute: mol What is the molar mass of the solute? molar mass: g / mol

The molar concentration is 0.0529 M

We have 0.0505 moles solute

The molar mass of the solute is 64.16 g/mol

Explanation:

Step 1: Data given

Mass of the  nonelectrolyte solute = 3.24 grams

Volume of water = 955 mL

Temperature = 22 °C = 295 K

Osmotic pressure = 973 torr = 973 / 760 = 1.28026 atm

Step 2: Calculate mass water

Mass water = 955 mL * 1g/mL

Mass water = 955 grams = 0.955 kg

Step 3: Calculate the molar concentration

π = i*M*R*T

⇒with π = the osmotic pressure = 1.28026 atm

⇒with i = the van't Hoff factor = 1

⇒with M = the molar concentration

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 295 K

M = 1.28026 / (0.08206*295)

M = 0.0529 M

Step 4: Calculate moles solute

Molar concentration = moles / volume

Moles solute = Molar concentration * volume

Moles solute = 0.0529 M * 0.955 L

Moles solute = 0.0505 moles

Step 5: Calculate molar mass

Molar mass = mass / moles

Molar mass = 3.24 grams / 0.0505 moles

Molar mass = 64.16 g/mol

The molar concentration is 0.0529 M

We have 0.0505 moles solute

The molar mass of the solute is 64.16 g/mol

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.