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nika2105 [10]
3 years ago
9

A chemical reaction yields 3 moles of lithium hydroxide (LiOH). How many grams of

Chemistry
1 answer:
grin007 [14]3 years ago
8 0

72g

Explanation:

Given parameters:

Number of moles of LiOH = 3moles

Unknown:

Mass of LiOH = ?

Solution:

A mole of  substance is a unit used to make quantitative measures in chemistry.

It is the amount of substance that contains the avogadro's number of particles.

The mole is related to mass using the expression below;

    Mass of a substance = number of moles x molar mass

Molar mass of LiOH = 7 + 16 + 1 = 24g/mol

 Mass of LiOH = 3 x 24 = 72g

learn more:

Number of moles brainly.com/question/1841136

#learnwithBrainly

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A sample of gas has an initial pressure of 1.5 atm, an initial volume of 3.0 L, and an initial temperature of 293K. If the final
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Answer:

1.9 L

Explanation:

Step 1: Given data

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  • Initial volume (V₁): 3.0 L
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Step 2: Calculate the final volume of the gas

If we assume ideal behavior, we can calculate the final volume of the gas using the combined gas law.

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Apart from plants, what other group of organisms photosynthesises?<br>​
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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
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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 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

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Converting the volume of laboratory to liter;

since 1 m³ = 100 L; Then, we  have:

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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}

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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}

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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.

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