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Trava [24]
2 years ago
9

Automotive airbags inflate when sodium azide NaN3 decomposes. In preparation of the

Chemistry
1 answer:
son4ous [18]2 years ago
8 0

63.1 g of NaN3 is formed when 50.0 g of sodium is reacted with 40.5 g of nitrogen according to the balanced chemical reaction

The balanced reaction equation is;

2 Na + 3 N2--> 2 NaN3

Number of moles of Na =  50.0 g/23 g/mol = 2.17 moles of Na

Number of moles of Nitrogen = 40.5 g/28 g/mol = 1.45 moles of N2

We have to obtain the limiting reactant, this is the reactant that yields the least number of moles of product.

For Na

2 moles of Na yields 2 moles of NaN3

2.17 moles of Na yields 2.17 moles of NaN3 (reaction is 1:1).

For N2

3 moles of N2 yields 2 moles of NaN3

1.45 moles of N2 yields 1.45 * 2/3 = 0.97 moles of NaN3

So, N2 is the limiting reactant. Mass of product formed depends on the limiting reactant.

Mass of NaN3 = 0.97 moles of NaN3 * 65 g/mol = 63.1 g of NaN3

Therefore, 63.1 g of NaN3 is formed when 50.0 g of sodium is reacted with 40.5 g of nitrogen according to the balanced chemical reaction

Learn more: brainly.com/question/9743981

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200.00 grams of an organic compound is known to contain 83.884 grams of carbon, 10.486
ololo11 [35]

The empirical formula of a given compound is C6H9ON5.

<u>Explanation</u>:

Step 1: Obtain the mass of each element present in grams

                  Element % = mass in g = m

Carbon = 83.884 grams, Hydrogen = 10.486 grams, Oxygen = 18.640 grams, Nitrogen = 86.99 grams.

Step 2: Determine the number of moles of each type of atom present

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Molar amount of carbon = (83.884 1 mol ) / 12 g = 6.99

Molar amount of hydrogen = (10.486  1 mol) / 1 g = 10.49

Molar amount of oxygen = (18.64  1 mol) / 16 g = 1.17

Molar amount of nitrogen = (86.99  1 mol) / 14 g = 6.21

Step 3: Divide the number of moles of each element by the smallest number of moles

            M / least M value = Atomic Ratio (R)

Atomic radius of carbon = 6.99 / 1.17 = 5.9 = 6

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Atomic radius of oxygen = 1.17 / 1.17 = 1

Atomic radius of nitrogen = 6.21 / 1.17 = 5

Step 4: Convert numbers to whole numbers. This set of whole numbers are the subscripts in the empirical formula.

            R * whole number = Empirical Formula

The empirical formula of a given compound is C6H9ON5.

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