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LuckyWell [14K]

3 years ago

5

The deployment of airbags during a car accident results from a chemical reaction that, until the 1990s, involved sodium azide, N

aN 3 . Sodium azide has since been replaced by less toxic substances that react in a similar way. In older airbags a crash triggers the decomposition of NaN 3 to form elemental sodium and nitrogen gas , which fills the airbag . How many moles of N 2 gas are produced when 167.7 g NaN 3 decomposes ?

1 answer:

stiks02 [169]3 years ago

4 0

Answer:

Number of moles of nitrogen produced from 167.7 g of sodium azide are 3.87.

Explanation:

Given data:

Mass of sodium azide = 167.7 g

Moles of nitrogen gas produced = ?

Solution:

First of all we will write the balance chemical equation of decomposition of sodium azide.

Chemical equation:

2NaN₃ → 3N₂ + 2Na

Number of moles of sodium azide:

Number of moles of sodium azide = mass / molar mass

Number of moles of sodium azide = 167.7 g/ 65 g/mol

Number of moles of sodium azide = 2.58 mol

Now we compare the moles of sodium azide with nitrogen from balance chemical equation.

NaN₃ : N₂

2 : 3

2.58 : 3/2×2.58 = 3.87

Number of moles of nitrogen produced from 167.7 g of sodium azide are 3.87.

Mass of nitrogen produced = moles × molar mass

Mass of nitrogen produced = 3.87 mol × 14 g/mol

Mass of nitrogen produced = 54.18 g.

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Solution :

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Thus, the value of 'x' will be, 0.0742 M

Now we have to calculate the equilibrium concentration of NO.

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3 years ago

How many moles are present in 3.4 x 1023 atoms of Na?

Andrej [43]

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7 0

2 years ago

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Answer:

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Explanation:

Step 1: Data given

rate = k[N2O]

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Step 3: Calculate the concentration of N2O after 2.0 minutes

We use the rate law to derive a time dependent equation.

-d[N2O]/dt = k[N2O]

ln[N2O] = -kt + ln[N2O]i

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3 years ago