A chemist accidentally leaves an open beaker containing 500.0 mL of a 0.250 M Mg(NO3)2(aq) solution on a lab bench. They return a few days later to find that the volume of the solution has decreased to 100.0 mL. What is the molarity of this partially evaporated solution, assuming the solute does not evaporate

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 :

i think it's c. if you look search electronic symbol on google and then click on wiki it shows you a