The sodium azide required for automobile air bags is made by the reaction of sodium metal...
The sodium azide required for automobile air bags is made by the reaction of sodium metal with dinitrogen monoxide in liquid ammonia: You have 62.8 g of sodium, a 35.5-L flask containing N2O gas with a pressure of 2.48 atm at 23 °C, and excess ammonia. What is the theoretical yield (in grams) of NaN3?
3 N2O (g) + 4 Na (s) + NH3 (l) ---> NaN3 (s) + 3 NaOH (s) + 2 N2 (g)
Mass = g
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The sodium azide required for automobile air bags is made by the
reaction of sodium metal...
de in agus asmoa The sodium azide required for automobile bags is made by the reaction...
de in agus asmoa The sodium azide required for automobile bags is made by the reaction of sodium metal with donutsoen mo 3 NO(8) + 4 Na(9) +NH ( + NaNa (8) + 3 NaOH(4) + 2 N3 (8) You have 59.4 g of sodium, 248.7.La conting N, O gas with a pressure of 2.93 atm 21 °C, and excess NaN3? monia. What is the theoretical yield (in grams) of Submit AS Try Another Version
10. (10 points) Sodium azide, NaNs, is used to provide gas to inflate automobile air bags....
10. (10 points) Sodium azide, NaNs, is used to provide gas to inflate automobile air bags. What mass of sodium azide is needed to provide the nitrogen needed to inflate a 70.0 L bag to a pressure of 1.3 atm at 25°C? 2 NaN3 (s) → 2 Na (s) + 3 N2(g)
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid...
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation 2 NaN3(s) - 2 Na(s) + 3 N2(9) Using stoichiometry and the ideal gas law, calculate the mass (ing) of NaN3 required to provide 42 L of N2(g) at 28.3 °C and 1.00 atm?
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid...
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) → 2 Na(s) + 3 N2(g). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 27.2 L of N2(g) at 44 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) + 2 H20(9). How many grams of water could be...
Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2...
Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) – 2 Na(s) + 3 N2(9). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 20 L of N2(g) at 38 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) → 2 H2O(g). How many grams of water could be produced by...
answer both questions pls!! QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to...
answer both questions pls!!
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) + 2 Na(s) + 3 N2(g). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 45.7 L of N2(g) at 41.4 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) + 2 H2O(g). How many grams...
1. Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed:...
1. Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed: 2NaN3 (s) ―—› 2Na(s) + 3N2(g) What mass of sodium azide is required to produce 2.6 ft3 (73.6 L) of nitrogen gas with a density of 1.25 g/L?
3&4 QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for...
3&4
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) 2 Na(s) + 3 N2(g) Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 30.3 L of N2(g) at 25.6 C and 1 00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water 2 H2(g) O2(a)-2 H20(g) How many grams of water could be produced by...
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition...
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3. 2 NaNz (s) + 2 Na (s) + 3 N2(g) If an air bag has a volume of 47.2 L and is to be filled with nitrogen gas at a pressure of 1.02 atm at a temperature of 24.1°C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas.
Automobile air bags inflate following a serious impact.
Automobile air bags inflate following a serious impact. The impact triggers the following chemical reaction:2 NaN3(s) → 2 Na(s)+3 N2(g)Part AIf an automobile air bag has a volume of 11.7 L, what mass of NaN3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.
de in agus asmoa The sodium azide required for automobile bags is made by the reaction of sodium metal with donutsoen mo 3 NO(8) + 4 Na(9) +NH ( + NaNa (8) + 3 NaOH(4) + 2 N3 (8) You have 59.4 g of sodium, 248.7.La conting N, O gas with a pressure of 2.93 atm 21 °C, and excess NaN3? monia. What is the theoretical yield (in grams) of Submit AS Try Another Version
10. (10 points) Sodium azide, NaNs, is used to provide gas to inflate automobile air bags. What mass of sodium azide is needed to provide the nitrogen needed to inflate a 70.0 L bag to a pressure of 1.3 atm at 25°C? 2 NaN3 (s) → 2 Na (s) + 3 N2(g)
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation 2 NaN3(s) - 2 Na(s) + 3 N2(9) Using stoichiometry and the ideal gas law, calculate the mass (ing) of NaN3 required to provide 42 L of N2(g) at 28.3 °C and 1.00 atm?
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) → 2 Na(s) + 3 N2(g). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 27.2 L of N2(g) at 44 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) + 2 H20(9). How many grams of water could be...
Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) – 2 Na(s) + 3 N2(9). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 20 L of N2(g) at 38 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) → 2 H2O(g). How many grams of water could be produced by...
answer both questions pls!!
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) + 2 Na(s) + 3 N2(g). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 45.7 L of N2(g) at 41.4 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) + 2 H2O(g). How many grams...
3&4
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) 2 Na(s) + 3 N2(g) Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 30.3 L of N2(g) at 25.6 C and 1 00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water 2 H2(g) O2(a)-2 H20(g) How many grams of water could be produced by...
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3. 2 NaNz (s) + 2 Na (s) + 3 N2(g) If an air bag has a volume of 47.2 L and is to be filled with nitrogen gas at a pressure of 1.02 atm at a temperature of 24.1°C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas.
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