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Firlakuza [10]
3 years ago
6

Write the correct term: In gaseous substances, the individual molecules are relatively (close/far apart) and are moving freely,

rapidly, and randomly.
Chemistry
1 answer:
GuDViN [60]3 years ago
3 0

Answer:

far apart

Explanation:

The molecules of any gaseous compounds are loosely bound and the molecules are far apart from each other. They move freely and rapidly. The inter-molecular forces are lower as compared to a solid or a liquid where the molecules are comparatively closely bound in the compounds.  

Because of the large gap or distance between its molecules, gaseous compounds have less density  when compared to any solid or liquid.

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1) A certain compound has an empirical formula of CH_6O_ 2. Its molar mass is between 285 and 315 g/mol. What is its molecular f
KIM [24]

1. The molecular formula of the compound is C₆H₃₆O₁₂

2. The molecular formula of the compound is N₂H₄O₂

3 The empirical formula and molecular formula of the compound are: C₂H₃ and C₄H₆

4. The empirical formula of the compound is C₃H₆O

5. The empirical formula of the compound is ZrSiO₄

<h3>1. How to determine the molecular formula </h3>
  • Empirical formula = CH₆O₂
  • Molar mass = (285 + 315) / 2 = 600 / 2 = 300 g/mole
  • Molecular formula =?

Molecular formula = empirical × n = molar mass

[CH₆O₂]ₙ = 300

[12 + (6×1) + (16×2)]ₙ = 300

50n = 300

Divide both side by 74

n = 300 / 50

n = 6

Molecular formula = [CH₆O₂]ₙ

Molecular formula = [CH₆O₂]₆

Molecular formula = C₆H₃₆O₁₂

<h3>2. How to determine the molecular formula </h3>
  • Empirical formula = NH₂O
  • Molar mass = (55 + 65) / 2 = 120 / 2 = 60 g/mole
  • Molecular formula =?

Molecular formula = empirical × n = molar mass

[NH₂O]ₙ = 60

[14 + (2×1) + 16]ₙ = 60

32n = 60

Divide both side by 32

n = 60 / 32

n = 2

Molecular formula = [NH₂O]ₙ

Molecular formula = [NH₂O]₂

Molecular formula = N₂H₄O₂

<h3>3. How to determine the empirical formula and molecular formula</h3>

We'll begin by obtaining the empirical formula. This is illustrated below:

  • Carbon (C) = 88.9%
  • Hydrogen (H) = 11.1%
  • Empirical formula =?

Divide by their molar mass

C = 88.9 / 12 = 7.4

H = 11.1 / 1 = 11.1

Divide by the smallest

C = 7.4 / 7.4 = 1

H = 11.1 / 7.4 = 3/2

Multiply by 2 to express in whole number

C = 1 × 2 = 2

H = 3/2 × 2 = 3

Thus, the empirical formula of the compound is C₂H₃

Finally, we shall determine the molecular formula of the compound. This is illustrated below:

  • Molar mass of compound = 54 g/mol
  • Empirical formula = C₂H₃
  • Molecular formula =?

Molecular formula = empirical × n = molar mass

[C₂H₃]ₙ = 75.16

[(12×2) + (3×1)]ₙ = 54

27n = 54

Divide both side by 27

n = 54 / 27

n = 2

Molecular formula = [C₂H₃]ₙ

Molecular formula = [C₂H₃]₂

Molecular formula = C₄H₆

<h3>4. How to determine the empirical formula</h3>
  • Carbon (C) = 62.07%
  • Hydrogen (H) = 10.34%
  • Oxygen (O) = 27.59%
  • Empirical formula =?

Divide by their molar mass

C = 62.07 / 12 = 5.1725

H = 10.34 / 1 = 10.34

O = 27.59 / 16 = 1.724

Divide by the smallest

C = 5.1725 / 1.724 = 3

H = 10.34 / 1.724 = 6

O = 1.724 / 1.724 = 1

Thus, the empirical formula of the compound is C₃H₆O

<h3>5. How to determine the empirical formula</h3>
  • Zr = 49.76%
  • Si = 15.32%
  • O = 34.91%
  • Empirical formula =?

Divide by their molar mass

Zr = 49.76 / 91 = 0.547

Si = 15.32 / 28 = 0.547

O = 34.91 / 16 = 2.182

Divide by the smallest

Zr = 0.547 / 0.547 = 1

Si = 0.547 / 0.547 = 1

O = 2.182 / 0.547 = 4

Thus, the empirical formula of the compound is ZrSiO₄

Learn more about empirical and molecular formula:

brainly.com/question/24297883

#SPJ1

7 0
2 years ago
1) A 10g sample of H2(g) reacts with a 22g sample of O2(g) according to
solmaris [256]

Answer:

H₂ is excess reactant and O₂ the limiting reactant

Explanation:

Based on the chemical reaction:

2H₂(g) + O₂(g) → 2H₂O

<em>2 moles of H₂ react per mole of O₂</em>

<em />

To find limiting reactant we need to convert the mass of each reactant to moles:

<em>Moles H₂ -Molar mass: 2.016g/mol-:</em>

10g H₂ * (1mol / 2.016g) = 4.96 moles

<em>Moles O₂ -Molar mass: 32g/mol-:</em>

22g O₂ * (1mol / 32g) = 0.69 moles

For a complete reaction of 0.69 moles of O₂ are needed:

0.69mol O₂ * (2mol H₂ / 1mol O₂) = 1.38 moles of H₂

As there are 4.96 moles,

<h3>H₂ is excess reactant and O₂ the limiting reactant</h3>
7 0
4 years ago
that B) My color is sickle: I have a drop of water in my body when I was given heat, white powder was formed So who am i Lets id
kramer

Explanation:

i don't understood your question ⁉️

and what do u mean by my color is sickle

8 0
3 years ago
Answer pls ASAPPP 50 pointsss!!
amm1812

Answer:

There should only be one chemical reaction, this is because toasting the bread is not only using heat, but you cannot untoast the bread, and also theres a reaction with the amino acids and sugar in bread when it's cooked. I hope this helps you! :)

5 0
3 years ago
Read 2 more answers
how do i word a formal letter to a teacher saying i didn't pay attention during the science lessons and i now have no idea what
Allushta [10]

Explanation:

Hello mr/mrs (name) I unfortunately couldn't pay attention to the class due to some issues I had therefore I don't know what we are doing in class

OR

Hello mr/mrs (name) I could understand what we were doing in class I would like it if you could break it down more or explain better to me

OR just say something it had something to do with your internet such as

Hello mr/mrs (name) I didn't understand what you were saying during our class due to some of my internet issues I was have throughout the day. I hope you can explain what we did during the class.

Those may be some of my excuses I've used before

they have worked for me:)

I don't know if that helped?:/

8 0
3 years ago
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