12,500 j of energy is added to 2.0 mol (36 g) of h2o as an ice sample at 0°c. the molar heat of fusion is 6.02 kj/mol. the specific heat of liquid water is 4.18 j/mol k. the molar heat of vaporization is 40.6 kj/mol. the resulting sample contains which of the following?

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 :

c. 4.54 x 10–12 j happens to be correct