Calculate the vapor pressure of a solution containing 24.6 g of glycerin (c3h8o3) in 134 ml of water at 30.0 ∘c. the vapor pressure of pure water at this temperature is 31.8 torr. assume that glycerin is not volatile and dissolves molecularly (i. e., it is not ionic) and use a density of 1.00 g/ml for the water.

Answer : The vapor pressure of a solution is, 30.687 torr

Explanation :

First we have to calculate the moles of glycerin.

Now we have to calculate the mass of water.

Now we have to calculate the moles of water.

Now we have to calculate the mole fraction of water.

Now we have to calculate the vapor pressure of the solution.

According to the Raoult's law,

where,

= vapor pressure of solution = ?

= vapor pressure of pure water= 31.8 torr

= mole fraction of water = 0.965

Now put all the given values in this formula, we get the vapor pressure of solution.

Therefore, the vapor pressure of a solution is, 30.687 torr

the law of conservation of mass states that in a chemical reaction, the total mass of reactants is equal to the total mass of products. because atoms are only rearranged in a chemical reaction, there must be the same number of sodium atoms and chlorine atoms in both the reactants and products