The vapor pressure of water at 65oc is 187.54 mmhg. what is the vapor pressure of a ethylene glycol (ch2(oh)ch2(oh)) solution made by dissolving 22.37 g of ethylene glycol in 82.21 g of water?

173.83 mmHg is the vapor pressure of a ethylene glycol solution.

Explanation:

Vapor pressure of water at 65 °C=

Vapor pressure of the solution at 65 °C=

The relative lowering of vapor pressure of solution in which non volatile solute is dissolved is equal to mole fraction of solute in the solution.

Mass of ethylene glycol = 22.37 g

Mass of water in a solution = 82.21 g

Moles of water=

Moles of ethylene glycol=

173.83 mmHg is the vapor pressure of a ethylene glycol solution.

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 :

the answer would be b i believe