Q5. Correct answer is : 0.88 g
Explanation
Given : mass NaN3 = 2.5 g
moles NaN3 = (mass NaN3) / (molar mass NaN3)
moles NaN3 = (2.5 g) / (65.0 g/mol)
moles NaN3 = 0.038455 mol
moles Na produced = moles NaN3 consumed
moles Na produced = 0.038455 mol
mass Na produced = (moles Na produced) * (molar mass Na)
mass Na produced = (0.038455 mol) * (23 g/mol)
mass Na produced = 0.88 g
How many grams of sodium are produced when 2.5 grams of sodium azide decomposes Drive -...
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?
Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2NaN3(s)?2Na(s)+3N2(g) How many moles of N2 are produced by the decomposition of 1.70 mol of NaN3?
Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements:2NaN3(s) → 2Na(s)+3N2(g)How many moles of N2 are produced by the decomposition of 3.55 mol of sodium azide?10.71.185.332.371.78
Automobile airbags contain sodium azide, NaN3. It decomposes to form sodium and nitrogen gas; the nitrogen inflates the airbag. How many grams of NaNg are needed to inflate an airbag to a volume of 65 Lat 2.5 atm and 25 °C?
Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s)→2Na(s)+3N2(g) How many grams of sodium azide are required to produce 30.5 g of nitrogen?
(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a canister: 2 NaN3(s) 2 Na(s) +3 N2(g) An average driver's side airbag has a volume of 52L. How many grams of NaN3 do you need to decompose to fill the airbag with N2 at room temperature (25°C) and atmospheric pressure (1.00 atm)?
Airbags uses the decomposition of sodium azide for inflation. How many moles of sodium azide, NaN3, would have to decompose to produce 253,000,000 molecules of nitrogen gas N2? 2NaN3(s) 2Na(s) + 3N2
When sensors in a car detect a collision, they cause the reaction of sodium azide, NaN3, which generates nitrogen gas to fill the air bags within 0.03 s. 2NaN3(s)→2Na(s)+3N2(g) How many liters of N2 are produced at STP if the air bag contains 101 g of NaN3? Express your answer with the appropriate units.
(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a canister: 2 NaN3(s) → 2 Na(s) + 3 N2(g) An average driver's side airbag has a volume of 52L. How many grams of NaNz do you need to decompose to fill the airbag with N2 at room temperature (25°C) and atmospheric pressure (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...