Car airbags inflate upon sudden deceleration due to the following chemical reaction: a) What is the value of ??? ?? 289 for NaN 3 ? b) A fully inflated airbag requires 2.4 mol of N 2 (g). Calculate the enthalpy change to fully inflate an airbag, which occurs when an airbag is fully inflated. c) Assuming all energy goes into heating the 2.4 mol of N 2 (g), what will the final temperature of the gas be? C p for N 2 (g) = 29.1 J K –1 mol -1 Solution Solution :- NaN3(s) ----> Na(s) + 3/2 N2(g)    delta H = -21.7 kJ/mol #a)Calculating the   value of delta Hfo of the NaN3(s) Delta Hrxn = sum of delta Hfo product - sum of delta Hfo reactant -21.7 kJ/mol= [(1*Na)+(3/2*N2)]-[1*NaN3] -21.7 kJ/mol = [(1*0)+(3/2*0)] - [1*NaN3] -21.7 kJ/mol = 0 - [1*NaN3] 21.7 kJ/mol = NaN3(s) Therefore the Delta Hfo of the NaN3(s) is 21.7 kJ/mol #b) fully inflate airbag contains 2.4 mol N2(g) As we know from the reaction equation (3/2) mol N2 gives -21.7 kJ energy So lets calculate the amount of energy given for the 2.4 mol N2 2.4 mol N2 * -21.7 kJ / (3/2) mol N2 = -34.72 kJ Therefore enthalpy change for the fully inflate airbag is -34.72 kJ #c) initial temperature of the gas should be 298 K Lets calculate the change in the temperature after Delta T = delta H/(n* Cp) Delta T= (34.72 kJ*1000 J/1kJ)/(2.4 mol * 29.1 J/mol K) = 497 K So the final temperature of the N2 gas will be 497 K .