Gaseous Nitrous oxide decomposes at 298 ~K to form Nitrogen gas and Oxygen gas. The H for the reaction at 1.0 ~atm pressure and 298 ~K is - 1 6 3 . 1 5 ~ k J . Calculate Internal energy change for the decomposition of 100 ~g of Nitrous oxide gas under the same conditions of temperature and pressure.

Step-by-step solution

The decomposition reaction of nitrous oxide is: 2N₂O(g) 2N₂(g) + O₂(g) . The molar mass of N₂O is 28 + 16 = 44 g/mol . The number of moles of N₂O in 100 g is n = 100 44 2.2727 mol . The enthalpy change for the decomposition of 2 moles of N₂O is given as H = -163.15 kJ . For n = 2.2727 moles , the enthalpy change H_ total is H_ total = ( -163.15 2 ) 2.2727 = -81.575 2.2727 -185.4 kJ . The relationship between enthalpy change and internal energy change is H = U + n_ g RT . For the reaction 2N₂O(g) 2N₂(g) + O₂(g) , th