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the chemical equation describing the overall reaction in an automobile bag: 20 NaN3(s)+6 Sio2(s)+4 KNOs(s)-32 N2(g)+5...
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)
The following is the reaction that occurs in automobile airbags: 2 NaN3(s)⟶ 2 Na(s) + 3 N2(g) How many grams of sodium azide (NaN3) are required to produce 19.00 L of N2 at 293K and 775 mm Hg?
Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2NaN3(s)→2Na(s)+3N2(g) a. How many moles of N2 are produced by the decomposition of 1.70 mol of NaN3? b. How many grams of NaN3 are required to form 13.0 g of nitrogen gas? c. How many grams of NaN3 are required to produce 11.0 ft3 of nitrogen gas if the gas has a density of 1.25 g/L?
Automobile air bags inflate during a crash or sudden stop by the rapid generation of nitrogen gas from sodium azide, according to the reaction: 2NaN, (s) + 2Na(s) +3N2 (8) V 1st attempt See Periodic Table D See Hint How many grams of sodium azide are needed to provide sufficient nitrogen gas to fill a 40.0 x 40.0 25.0 cm bag to a pressure of 1.13 atm at 23.0 °C? g sodium azide
Automobile air bags inflate during a crash or sudden stop by the rapid generation of nitrogen gas from sodium azide, according to the reaction: 2NaN(s) —→ 2Na(s) + 3N, (g) v 4th attempt i See Periodic Table D See How many grams of sodium azide are needed to provide sufficient nitrogen gas to fill a 40.0 x 40.0 25.0 cm bag to a pressure of 1.21 atm at 23.0°C? 79.34 g sodium azide
Automobile air bags inflate during a crash or sudden stop by the rapid generation of nitrogen gas from sodium azide, according to the reaction: 2NaN3 (s) 2Na (s) + 3N2 (g) How many grams of sodium azide are needed to provide sufficient nitrogen gas to fill a 40.0 × 40.0 × 25.0 cm bag to a pressure of 1.13 atm at 23.0 °C?
Automobile air bags inflate during a crash or sudden stop by the rapid generation of nitrogen gas from sodium azide, according to the reaction: 2NaN3(s) -----2Na(s)+3N2(g) How many grams of sodium azide are needed to provide sufficient nitrogen gas to fill a 30.0 × 30.0 × 25.0 cm bag to a pressure of 1.07 atm at 12.0 °C?
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...
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...
Name TUTTI Chemistry 219 Homework Assignment #12 - Physical States of Matter & som Matter & Solutions Atoms Focused Approach, 2 ed. by libert, NOS Kead and outline Chapter 10.6.10.10 of Chemistrn Foster, & Bretz as directed by your instructor. Ideal Gases and the Gas Laws 1. How many moles of air must there be in a racing bicycle tire with a volume of 2.36 L if it has an internal pressure of 6.8 atm at 17.0°C? (10.69) 2. The...