Automotive air bags inflate when sodium azide NaN3 decomposes. In preparation of the airbag a scientist reacts sodium with nitrogen to obtain sodium azide:
A) Balance the chemical reaction of this process:

Na (s) + ___N2 (g) → ___NaN3 (s)
B) If 50.0 g of sodium is reacted with 40.5 g of nitrogen according to the balanced chemical
reaction above what is the mass of sodium azide that can be obtained?
C) What is the limiting reagent in the reaction?
D) How much excess reagent left over when the reaction is complete?
E) What is the percent yield if the scientist obtained 34.5 g of sodium azide? Was this reaction
successful?

13. calculate the initial concentration (before precipitation) of carbonate ions after the addition of each 0.05 ml of solution b to the 1.00 l beaker of solution a. divide the work among group members and write the answers in the table in model 3. assume the volume change as solution b is added is negligible. 14. notice the initial concentrations of zn2+ - and cu2+ in the table in model 3. a. explain how these were obtained from the data in model 2. b. as solution b is added and precipitates form, do these initial concentrations change? 15. use the data in model 2 to indicate the presence of precipitate (either znco3 or cuco3) after each 0.05 ml addition of solution b in model 3. 16. use the initial concentrations of carbonate ions and zinc ions to calculate the reaction quotient, qsp for the zinc carbonate scenarios in model 3. divide the work among group members and write the answers in the table in model 3. 17. use the initial concentrations of carbonate ion and copper(ii) ions to calculate the qsp for the copper(ii) carbonate scenarios in model 3. divide the work among group members and write the answers in the table in model 3.