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azamat
3 years ago
6

Which phase has the most space between the particles? A.solid B.gas C.liquid

Chemistry
2 answers:
jonny [76]3 years ago
8 0

Answer:

B. gas

Explanation:

<em>The particles of matter in the gaseous state are neither close together nor fixed in place. The gas expands to fill its container. Thus, a given number of particles will have the </em><em>m</em><em>o</em><em>s</em><em>t</em><em> </em><em>s</em><em>p</em><em>a</em><em>c</em><em>e</em><em> </em><em>b</em><em>e</em><em>t</em><em>w</em><em>e</em><em>e</em><em>n</em><em> </em><em>t</em><em>h</em><em>e</em><em>m</em><em> in the gas state</em><em>.</em>

Brums [2.3K]3 years ago
8 0
B) gas
hope this helps x
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In the presence of a strong acid, litmus paper exhibits a(n) _________________ color.
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Why are silver, lead, and mercury so special? (why do they always precipitate out and never dissolve) PLEASE BE DETAILED BUT SIM
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Silver and lead are special elements, where silver is insoluble in all halogen anions (like AgCl, AgI, AgBr)
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3 years ago
Rusting of iron is a very common chemical reaction. It results in one form from Fe reacting with oxygen gas to produce iron (III
Vlada [557]

<u>Answer:</u> The given amount of iron reacts with 9.0 moles of O_2 and produce 6.0 moles of Fe_2O_3

<u>Explanation:</u>

We are given:

Moles of iron = 12.0 moles

The chemical equation for the rusting of iron follows:

4Fe+3O_2\rightarrow 2Fe_2O_3

  • <u>For oxygen gas:</u>

By Stoichiometry of the reaction:

4 moles of iron reacts with 3 moles of oxygen gas

So, 12.0 moles of iron will react with = \frac{3}{4}\times 12.0=9.0mol of oxygen gas

  • <u>For iron (III) oxide:</u>

By Stoichiometry of the reaction:

4 moles of iron produces 2 moles of iron (III) oxide

So, 12.0 moles of iron will produce = \frac{2}{4}\times 12.0=6.0mol of iron (III) oxide

Hence, the given amount of iron reacts with 9.0 moles of O_2 and produce 6.0 moles of Fe_2O_3

5 0
3 years ago
What is the empirical formula of a compound with a percent composition of 22.5% Phosphorous and 77.5% Chlorine?
sashaice [31]

Answer:

\boxed {\boxed {\sf PCl_3}}

Explanation:

We are given the percent composition: 22.5% phosphorus and 77.5% chlorine.

We can assume there are 100 grams of this compound. We choose 100 because we can simply use the percentages as the masses.

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  • 77.5 g Cl

Next, convert these masses to moles, using the molar masses found on the Periodic Table.

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  • Cl: 35.45 g/mol

Use the molar masses as ratios and multiply by the number of grams. 22.5 \ g \ P  * \frac {1 \ mol \ P }{30.974 \ g \ P}= \frac {22.5 \ mol \ P }{ 30.974} = 0.7264157035 \ mol \ P

77.5 \ g \ Cl  * \frac {1 \ mol \ Cl }{35.45 \ g \ Cl}= \frac {77.5 \ mol \ Cl }{ 35.45} \ =2.186177715 \ mol \ Cl

Divide both of the moles by the smallest number of moles to find the mole ratio.

\frac {0.7264157035} {0.7264157035} = 1

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The mole ratio is about 1 P: 3 Cl, so the empirical formula is written as:<u> PCl₃</u>

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