Asucrose solution is prepared to a final concentration of 0.190 m . convert this value into terms of g/l, molality, and mass % (molecular weight, mwsucrose = 342.296 g/mol ; density, ρsol′n = 1.02 g/ml ; mass of water, mwat = 955.0 g ). note that the mass of solute is included in the density of the solution.

The strength of the sucrose solution is 65.03624 g/L.

Molality of the solution is 0.1989 mol/kg.

Mass percentage of the solution is 6.37%

Explanation:

Strength of the sucrose solution

Molarity of the sucrose solution = 0.190 M = 0.190 mol/L

Molar mass of sucrose = 342.296 g/mol

Strength of the solution =  Molarity of the solution × Molar mass of the solute

Strength of the sucrose solution =

=

Molality of the solution:

Moles of sucrose in 1L solution = 0.190 moles

Mass of water = 955.0 g = 0.9550 kg

Molality of the solution is:

Mass percentage of the solution:

Density iof the solution =

Mass of solution = Mass of solute + Mass of water

Volume of solution = 1L = 1,000 mL

Mass of solution = 1.02 g/mL × 1,000 mL = 1,020 g

Mass of solute + Mass of water = 1,020 g

Mass of solute = 1,020 g - 955.0 g = 65.0 g

Mass percentage:

Mass percentage of the solution is 6.37%

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :