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almond37 [142]
2 years ago
9

What is the ratio of phosphorous atoms to oxygen atoms

Chemistry
1 answer:
ozzi2 years ago
6 0
2:5 is the answer have a awesome day
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If you place 1.0 L of ethanol (C2H5OH) in a small laboratory that is 3.0 m long, 2.0 m wide, and 2.0 m high, will all the alcoho
ankoles [38]

If you place 1.0 L of ethanol (C2H5OH) in a small laboratory that is 3.0 m long, 2.0 m wide, and 2.0 m high, will all the alcohol evaporate? If some liquid remains, how much will there be? The vapor pressure of ethyl alcohol at 25 °C is 59 mm Hg, and the density of the liquid at this temperature is 0.785g/cm^3 .

will all the alcohol evaporate? or none at all?

Answer:

Yes, all the ethanol present in the laboratory will evaporate since the mole of ethanol present in vapor is greater. The volume of ethanol left will therefore  be zero.

Explanation:

Given that:

The volume of alcohol which is placed in a small laboratory = 1.0 L

Vapor pressure of ethyl alcohol  at 25 ° C = 59 mmHg

Converting 59 mmHg to atm ; since 1 atm = 760 mmHg;

Then, we have:

= \frac{59}{760}atm

= 0.078 atm

Temperature = 25 ° C

= ( 25 + 273 K)

= 298 K.

Density of the ethanol = 0.785 g/cm³

The volume of laboratory = l × b × h

= 3.0 m × 2.0 m × 2.5 m

= 15 m³

Converting the volume of laboratory to liter;

since 1 m³ = 100 L; Then, we  have:

15 × 1000 = 15,000 L

Using ideal gas equation to determine the moles of ethanol in vapor phase; we have:

PV = nRT

Making n the subject of the formula; we have:

n = \frac{PV}{RT}

n = \frac{0.078 * 15000}{0.082*290}

n = 47. 88 mol of ethanol

Moles of ethanol in 1.0 L bottle can be calculated as follows:

Since  numbers of moles = \frac{mass}{molar mass}

and mass = density × vollume

Then; we can say ;

number of moles = \frac{density*volume }{molar mass of ethanol}

number of moles =\frac{0.785g/cm^3*1000cm^3}{46.07g/mol}

number of moles = \frac{&85}{46.07}

number of moles = 17.039 mol

Thus , all the ethanol present in the laboratory will evaporate since the mole of ethanol present in vapor is greater. The volume of ethanol left will therefore be zero.

5 0
2 years ago
In a metal what is not given an assigned location and thus can drift
Allushta [10]
In a metal, "Electrons" <span> is not given an assigned location and thus can drift

In short, Your Answer would be Option C

Hope this helps!</span>
6 0
2 years ago
How is electrolysis most commonly used to produce an energy source?
elena-s [515]

Answer:

Splitting water molecules produces hydrogen gas, which is used to power machines through hydrogen fuel cells. ( B-)

4 0
2 years ago
What is redox reaction??<br><img src="https://tex.z-dn.net/?f=%20%5C%5C%20%20%5C%5C%20" id="TexFormula1" title=" \\ \\ " alt="
MAXImum [283]

Answer:

Oxidation–reduction or redox reactions are reactions that involve the transfer of electrons between chemical species (check out this article on redox reactions if you want a refresher!). The equations for oxidation-reduction reactions must be balanced for both mass and charge, which can make them challenging to balance by inspection alone. In this article, we’ll learn about the half-reaction method of balancing, a helpful procedure for balancing the equations of redox reactions occurring in aqueous solution.

Explanation:

8 0
3 years ago
Read 2 more answers
a gas in a container with a fixed volume was originally at a pressure of 317kpa and a temperature of 154k. what is the new press
goldfiish [28.3K]
<h2>Hello!</h2>

The answer is: 4.77atm

<h2>Why?</h2>

Since there's a fixed volume, we can use the the Gay-Lussac's Law which stablish a relation between the pressure and the temperature:

\frac{P}{T}=k

<em>P</em> is the volume of the gas

<em>t</em> is the temperature of the gas

<em>k </em>is the proportionality constant

We also have the following equation:

\frac{P1}{T1}=\frac{P2}{T2}

Where:

P2=\frac{P1*T2}{T1}=\frac{317kPa*235K}{154K}=483.73kPa

We are asked to find the pressure in atm, so we must convert 483.73kPa to atm:

1kPa=0.009869atm

Then,

483.733kPa*\frac{0.009869atm}{1kPa}=4.77atm

Have a nice day!

8 0
3 years ago
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