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sdas [7]
3 years ago
11

What is the purpose of taller emissions stacks in industrial settings? a) They are intended to release particulates where there

is more wind to carry them away, but this also spreads pollution more widely. b) They allow chemical reactions to take place within the stack, thus creating less harmful particulates to be released from the stack. c) The taller emissions stack are a government requirements of the Clean Air Act Amendment, only serving the purpose of compliance to the law d) The particulates typically cannot be carried up in the airstream of a taller stack, so are naturally captured by gravity within the facility producing the pollution e) the taller emission stacks are meant to emit pollutants in a height where they are no longer pollutants any more
Chemistry
2 answers:
dusya [7]3 years ago
5 0
The correct option is A.
As part of the Clean Air Amendment, the government mandated industries to build emission stacks, through which pollutant can be released high into the air in order to prevent pollution of the local community. But this had resulted into interstate pollution, because at high altitudes, the wind carry the pollutants far away into other states or areas.

marissa [1.9K]3 years ago
5 0

the correct anwser is A

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Problem PageQuestion The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium
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Answer:

1. 2NaN₃(s) → 2Na(s) + 3N₂(g)

2. 14.5 g NaN₃

Explanation:

The answer is incomplete, as it is missing the required values to solve the problem. An internet search shows me these values for this question. Keep in mind that if your values are different your result will be different as well, but the solving methodology won't change.

" The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large volumes of nitrogen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid sodium azide (NaN₃) into solid sodium and gaseous dinitrogen. 2. Suppose 71.0 L of dinitrogen gas are produced by this reaction, at a temperature of 16.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must have reacted. Round your answer to 3 significant digits. "

1. The <u>reaction that takes place is</u>:

  • 2NaN₃(s) → 2Na(s) + 3N₂(g)

2. We use PV=nRT to <u>calculate the moles of N₂ that were produced</u>.

P = 1 atm

V = 71.0 L

n = ?

T = 16.0 °C ⇒ 16.0 + 273.16 = 289.16 K

  • 1 atm * 71.0 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 289.16 K
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Now we <u>convert N₂ moles to NaN₃ moles</u>:

  • 0.334 mol N₂ * \frac{2molNaN_{3}}{3molN_2} = 0.223 mol NaN₃

Finally we <u>convert NaN₃ moles to grams</u>, using its molar mass:

  • 0.223 mol NaN₃ * 65 g/mol = 14.5 g NaN₃

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dmitriy555 [2]

Answer:

Hello!

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Hope that Helps! Have A Wonderful Day! ☺

Explanation:

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D) Distillation is the process used to separate a solid from a liquid through <span>evaporating the liquid..</span>
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