(a) The mixture of chemicals contains sodium azide (NaN_(3)) which decomposes on heating to form sodium and nitrogen. 2NaN_(2)arrow 2Na+3N_(2) A typical air bag contains 130 g of sodium azide. (i) Calculate the mass of nitrogen that would be produced when 130 g of sodium azide decomposes. Relative atomic masses (A_(i)):N=14;Na=23 __ Mass of nitrogen=

1. We must understand the chemical reaction rst: . From the reaction equation, we can conclude that 2 mol of sodium azide (NaN3) produces 3 mol of nitrogen (N2).2. This problem requires us to calculate the mass of nitrogen produced when 130g of sodium azide decomposes. 3. Next, we need to calculate the molar mass of sodium azide: the atomic mass of sodium is 23g/mol, and the atomic mass of nitrogen is 14g/mol; Azide comprises one atom of sodium and three atoms of Nitrogen, thus the molar mass is calculation to be: 23 + (14 x 2 x 3) = 23 + 84 = 107 g/mol.4. Calculate the number of moles of sodium azide using the formula n = m/M (where n is the number of moles, m is the mass and M is the molar mass), we calculate .5. Molar qualitative relationship derived from the reaction equation: 2 mol sodium azide produces 3 mol nitrogen, so 1 mol sodium azide can produce 1.5 mol nitrogen.6. Using this ratio, we then determine the amount of nitrogen produced by 1.21 mol of sodium azide: 1.21 x 1.5 = 1.817425 moles of nitrogen.7. Nitrogen molecules are twin-atomic, which means every mole of nitrogen produces two moles of nitrogen atoms. Since the atomic weight of nitrogen is 14 g/mol, As a result, 1 mol of nitrogen molecules consists of of nitrogen.8. Hence, to convert the moles of nitrogen molecules into mass, the equation is: Mass of nitrogen = number of moles * molar mass. From our calculation, Mass of nitrogen =