Automobile airbags contain solid sodium azide, NaN3, that reacts to produce nitrogen gas when heated, thus inflating the bag. 2NaN 3 (s)----> 2Na(s) + 3N 2 (g). Calculate the value of work, w, for the following system if 34.5 g of NaN3 reacts completely at 1.00 atm and 22 °C.

Question: Automobile airbags contain solid sodium azide, NaN3, that reacts to produce nitrogen gas when heated, thus inflating the bag. 2NaN3(s) ----> 2Na(s) + 3N2(g) Calculate the value of w (work) for the following system if 20.2 g of NaN3 reacts completely at 1.00 atm and 22 degrees

How many grams of sodium azide (NaN3) are required to produce 19.00 L of N at 293K and 775 mm Hg? The safety airbags in automobiles are inflated by nitrogen gas generated by the rapid decomposition of sodium azide. NaN3(s) arrow Na(s) + N2(g) How many grams of sodium azide are needed to generate 60.0 L of N2 at 1 atm and 26 degrees Celsius?

Reaction I: 2 NaN3 \rightarrow 2Na + 3 N2 How many grams of NaN3 must be included in the canister to produce 67.0 L of nitrogen gas at a pressure of 100 kPa and 25.0 ^oC? What mass of the by-product, sodium metal, is produced in reaction I when the 67.0; Consider the decomposition of solid sodium azide, NaN_3, into sodium metal and nitrogen gas.

An air bag is deployed by utilizing the following reaction (the nitrogen gas produced inflates the air bag): If 10.5 g of NaN3 is decomposed, what theoretical mass of sodium should be produced? If only 2.84 g of sodium is actually collected, Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed.

How many grams of NaN3 are required to form 15.0 ft3 of nitrogen gas, about the size of an automotive airbag, if the gas has a density of 1.25 g/L? 2NaN3(s) arrow 2Na(s) + 3N2(g) If an automobile airbag has a volume of 11.3 L, what mass of NaN3 (in grams) is required to fully inflate the airbag upon impact? Assume STP conditions.

Airbags in cars contain sodium azide, NaN3, and inflate within 50ms upon reaction of the sodium azide, which breaks down into sodium metal and nitrogen gas. Calculate the work involved if 121g of NaN3 reacts inside an initially uniflated airbag in a car at 22.3 degrees C against a constant external atmospheric pressure of 98.7 kPa.

The balanced chemical equation for this reaction is 2 NaN3(s) gives 2 Na(l) + 3 N2(g). Given 62.5 grams of NaN3, what volume of; 2NaN3 (s) → 2Na (s) + 3N2 (g) A) How many moles of N2 are produced by the decomposition of 1.50 mol of NaN3? B) How many grams of NaN3 are required to form 5.0 (g) of nitrogen gas?

Question: Car airbags are inflated by a thermal decomposition of the sodium azide (NaN3) that yields nitrogen gas and sodium metal. 2NaN3(s) 2Na(s)+3N2(g) How many liters of nitrogen gas can be prepared from 2.30mol of NaN3 at 273.15K and 1.00atm. Assume ideal gas behavior. Use R=0.08206L atm/mol K for the ideal gas constant.

Question: Air bags in automobiles inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2NaN3(s) ----> 2Na(s) +3N2(g). A) How many moles of N2 are formed by the decomposition of 1.60 mol of NaN3? B) How many …