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natima [27]
3 years ago
5

Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2NaN3(s)→2Na(s)+3N2(g)

Chemistry
1 answer:
Brums [2.3K]3 years ago
8 0

Answer:

\boxed{\text{(a) 2.85 mol; (b) 21.7 g; (c) 712 g}}

Explanation:

We will need a balanced chemical equation with molar masses, volumes, and concentrations, so, let's gather all the information in one place.

M_r:     65.01                         28.01

         2NaN₃(s) ⟶ 2Na(s) + 3N₂(g)

n/mol:   1.90

m/g:                                        14.0

(a) Moles of N₂

The molar ratio is 3 mol N₂ = 2 mol NaN₃

\text{Moles of N}_{2} = \text{1.90 mol NaN$_{3}$}\times \dfrac{\text{3 mol N}_{2}}{\text{2 mol NaN$_{3}$}}= \textbf{2.85 mol N}_{2}\\\\\text{The reaction produces $\boxed{\textbf{2.85 mol N}_{2}}$}

(b) Mass of NaN₃

(i) Moles of N₂

\text{Moles of N}_{2} = \text{14.0 g N}_{2} \times \dfrac{\text{1 mol N}_{2}}{\text{ 28.01 g N}_{2}} = \text{0.4998 mol N}_{2}

(ii) Moles of NaN₃

\text{Moles of NaN}_{3} =\text{0.4998 mol N}_{2} \times \dfrac{\text{2 mol NaN}_{3}}{\text{3 mol N}_{2}} = \text{0.3332 mol NaN}_{3}

(iii) Mass of NaN₃

\text{Mass of NaN}_{3} = \text{0.3332 mol NaN}_{3} \times \dfrac{\text{65.01 g NaN}_{3}}{\text{1 mol NaN}_{3}} =\textbf{21.7 g NaN}_{3}\\\\\text{You must use }\boxed{\textbf{21.7 g NaN}_{3}}

(c)Mass of NaN₃

(i) Volume of N₂

V = \text{13.0 ft}^{3} \times \dfrac{\text{28.32 L}}{\text{1 ft}^{3}} = \text{368.2 L}

(ii) Mass of N₂

\text{Mass of N}_{2} = \text{368.2 L N}_{2} \times \dfrac{\text{1.25 g N}_{2}}{\text{1 L N}_{2}} = \text{460.2 g N}_{2}

(iii) Moles of N₂

\text{Moles of N}_{2} = \text{460.2 g N}_{2} \times \dfrac{\text{1 mol N}_{2}}{\text{ 28.01 g N}_{2}} = \text{16.43 mol N}_{2}

(iv) Moles of NaN₃

\text{Moles of NaN}_{3} =\text{16.43 mol N}_{2} \times \dfrac{\text{2 mol NaN}_{3}}{\text{3 mol N}_{2}} = \text{10.95 mol NaN}_{3}

(v) Mass of NaN₃

\text{Mass of NaN}_{3} = \text{10.95 mol NaN}_{3} \times \dfrac{\text{65.01 g NaN}_{3}}{\text{1 mol NaN}_{3}} =\textbf{712 g NaN}_{3}\\\\\text{You must use }\boxed{\textbf{712 g NaN}_{3}}

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Draw a structural formula for the alkene you would use to prepare the alcohol shown by hydroboration/oxidation.
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Answer:

See explanation

Explanation:

The question is incomplete because the image of the alcohol is missing. However, I will try give you a general picture of the reaction known as hydroboration of alkenes.

This reaction occurs in two steps. In the first step, -BH2 and H add to the same face of the double bond (syn addition).

In the second step, alkaline hydrogen peroxide is added and the alcohol is formed.

Note that the BH2 and H adds to the two atoms of the double bond. The final product of the reaction appears as if water was added to the original alkene following an anti-Markovnikov mechanism.

Steric hindrance is known to play a major role in this reaction as good yield of the anti-Markovnikov like product is obtained with alkenes having one of the carbon atoms of the double bond significantly hindered.

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An element A has an atomic number of 11 and another element B has an atomic number 17 (A
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2 years ago
Suppose that on a dry, sunny day when the air temperature is near 37 ∘C,37 ∘C, a certain swimming pool would increase in tempera
ioda

Answer:

The fraction of water body necessary to keep the temperature constant is 0,0051.

Explanation:

Heat:

Q=m*Ce*ΔT

Q= heat  (unknown)

m= mass  (unknown)

Ce= especific heat (1 cal/g*°C)

ΔT= variation of temperature  (2.75 °C)  

Latent heat:

ΔE=∝mΔHvap

ΔE= latent heat

m= mass  (unknown)

∝= mass fraction (unknown)

ΔHvap= enthalpy of vaporization (539.4 cal/g)

Since Q and E are equal, we can match both equations:

m*Ce*ΔT=∝*m*ΔHvap

Mass fraction is:

∝=\frac{Ce*ΔT}{ΔHvap}

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7 0
2 years ago
2AlF3 + 3K2O → 6KF + Al2O3<br><br> How many grams of AlF3would it take to make 15.524 g of KF?
mr_godi [17]
<h3>Answer:</h3>

7.4797 g AlF₃

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right

<u>Chemistry</u>

<u>Stoichiometry</u>

  • Reading a Periodic Table
<h3>Explanation:</h3>

<u>Step 1: Define</u>

[RxN] 2AlF₃ + 3K₂O → 6KF + Al₂O₃

[Given] 15.524 g KF

<u>Step 2: Identify Conversions</u>

[RxN] 2 mol AlF₃ = 6 mol KF

Molar Mass of Al - 26.98 g/mol

Molar Mass of F - 19.00 g/mol

Molar Mass of K - 39.10 g/mol

Molar Mass of AlF₃ - 26.98 + 3(19.00) = 83.98 g/mol

Molar Mass of KF - 39.10 + 19.00 = 58.10 g/mol

<u>Step 3: Stoichiometry</u>

  1. Set up:                              \displaystyle 15.524 \ g \ KF(\frac{1 \ mol \ KF}{58.10 \ g \ KF})(\frac{2 \ mol \ AlF_3}{6 \ mol \ KF})(\frac{83.98 \ g \ AlF_3}{1 \ mol \ AlF_3})
  2. Multiply/Divide:                                                                                                    \displaystyle 7.47966 \ g \ AlF_3

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 5 sig figs.</em>

7.47966 g AlF₃ ≈ 7.4797 g AlF₃

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