202.0 g of Borax (Na2B4O7) is dissolved in 400. mL of water. The density of water is 1.00 g/mL. Calculate the molarity of the solution (moles of solute/ liters of solution). Round molar masses to whole numbers, use appropriate significant figures, and show your work.

i believe it is c.) 1575 j.

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 :