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.

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? When car sensors detect a collision, they cause the reaction of sodium azide, NaN3, which generates nitrogen gas to fill the air bags within 0.03 s.

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?

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?

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.

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.

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.

An automobile airbag inflates when NaN3 is converted to Na + N2 ----- 2 NaN3 ----- 2 Na + 3 N2, what volume of N2 would be produced if 100 grams of NaN3 completely reacted at STP? A chemist determines by measurements that 0.040 moles of nitrogen gas participate in a chemical reaction. Calculate the mass of nitrogen gas that participates.

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 …

The impact of a collision triggers the decomposition of NaN3 as follows: 2NaN3(s) → 2Na(s) + 3N2(g). The nitrogen gas produced quickly inflates the bag between the driver and the windshield and dashboard. Calculate the volume of N2 generated at 80°C and 823 mmHg by the decomposition of 60.0 g of NaN3. (Answer: V = 36.9 L)