What volume of water (solute) (d = 1.00 g/ml) should be added to 600. ml of ethanol (solvent, c2h5oh) in order to have a solution that boils at 95.0°c? [for ethanol, kb = 1.22 °c/m, density = 0.789 g/ ml, boiling point = 78.4°c]

Volume of water to be added is 116 ml.

Explanation:

Elevation in boiling point is given by:

= elevation in boiling point

i= vant hoff factor = 1 (for non electrolyte)

=boiling point constant =

m= molality

Density of solvent =

   (1kg=1000g)

Mass of solute (water) = x g

Density of solute =

Thus the volume of water to be added is 116 ml.

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 :