Liquid A has a vapor pressure of 7.37 kPa at 40C. Liquid B has a vapor pressure of 18.04kPa at 40C. Which liquid would evaporate faster at 40C? Explain your answer.

Liquid B because of its higher vapor pressure due to the fact that evaporation rate is directly proportional to vapor pressure

Explanation:

The vapor pressure of  liquid at equilibrium is a function to the liquid's rate of evaporation. The evaporation rate and hence the vapor pressure is a measure of the propensity of the particles  of the liquid to leave the surface of the liquid and exist as vapor directly above the liquid. As high evaporation rate leads to high vapor pressure, a liquid with a higher vapor pressure will evaporate faster than one with a lower vapor pressure at the same temperature and pressure.

Therefore, liquid B with a vapor pressure of 18.04 kPa at 40° C will evaporate faster than liquid A with a lower vapor pressure of 7.37 kPa at the same 40°C.

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 :

thats a little if u want the answer just look it up on google thats what i do haha : )