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4 years ago

CHEM HELP!

Chemistry

1 answer:

sweet [91]4 years ago

4 0

So let's convert this amount of mL to grams:

$\frac{13.6g}{1mL}*1.2mL=16.32g$

Then we need to convert to moles using the molar weight found on the periodic table for mercury (Hg):

$\frac{1mole}{200.59g}*16.32g=8.135*10^{-2}mol$

Then we need to convert moles to atoms using Avogadro's number:

$\frac{6.022*10^{23}atoms}{1mole} *[8.135*10^{-2}mol]=4.90*10^{22}atoms$

So now we know that in 1.2 mL of liquid mercury, there are $4.90*10^{22}atoms$ present.

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Do the gas laws apply to liquids ?

Contact [7]

Answer:

The Ideal Gas Law cannot be applied to liquids. The Ideal Gas Law is #PV = nRT#. That implies that #V# is a variable. But we know that a liquid has a constant volume, so the Ideal Gas Law cannot apply to a liquid.

Explanation:

this is my awnser soory if it was a multiple choice question plz mark brainliest

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3 years ago

Read 2 more answers

If a molecule can hydrogen bond does it guarantee that it will have a higher boiling point than a molecule that cannot?

sleet_krkn [62]

A molecule that can h-bond will not always necessarily and does not have guarantee to have a higher boiling point than one than cannot have h-bond.
we can take an example of Pentan-2-one that cannot h-bond but instead of this it has a high boiling point that is 102.3 °C, while propan-1-ol can h-bond but it has a boiling point of 97.2°C, that is lower than the boiling point of Pentan-2-one.

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4 years ago

Two categories of compounds are

crimeas [40]

Answer is: (3) ionic and molecular.

Ionic compounds are made of ions held together with ionic bonds.

Ionic bond forms when a cation transfers its extra electron to an anion who needs it.

For example compound magnesium chloride (MgCl₂) has ionic bond (the electrostatic attraction between oppositely charged ions).

Magnesium (metal) transfers two electrons (became positive cation) to chlorine (became negative anion).

Molecular compounds are made up of molecules whose atoms are connected with covalent bonds.

Covalent bond is bond between nonmetals.

For example, molecule carbon monoxide CO has covalent bond.

Carbon (C) and oxygen (O) are nonmetals.

Carbon atom and oxygen atom are connected by a triple bond (six shared electrons in three bonding molecular orbitals) that is formed of two covalent bonds and one dative covalent bond.

4 0

3 years ago

Read 2 more answers

How do the two desalination processes differ from the atmospheric water generator in terms of where the processes can be used?

-Dominant- [34]

Water Desalination Processes. Water desalination processes separate dissolved salts and other minerals from water. Feedwater sources may include brackish, seawater, wells, surface (rivers and streams), wastewater, and industrial feed and process waters. Membrane separation requires driving forces including pressure (applied and vapor),...

Hope I helped :)

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3 years ago

Three 1.0-l flasks, maintained at 308 k, are connected to each other with stopcocks. initially the stopcocks are closed. one of

Licemer1 [7]

Answer:

0.6103 atm.

Explanation:

We need to calculate the vapor pressure of each component after the stopcocks are opened.

Volume after the stopcocks are opened = 3.0 L.

1) For N₂:

P₁V₁ = P₂V₂

P₁ = 1.5 atm & V₁ = 1.0 L & V₂ = 3.0 L.

P₂ of N₂ = P₁V₁ / V₂ = (1.5 atm) (1.0 L) / (3.0 L) = 0.5 atm.

2) For H₂O:

Pressure of water at 308 K is 42.0 mmHg.

we need to convert from mmHg to atm: (1.0 atm = 760.0 mmHg).

P of H₂O = (1.0 atm x 42.0 mmHg) / (760.0 mmHg) = 0.0553 atm.

We must check if more 2.2 g of water is evaporated,

n = PV/RT = (0.0553 atm) (3.0 L) / (0.082 L.atm/mol.K) (308 K) = 0.00656 mole.

m = n x cmolar mass = (0.00656 mole) (18.0 g/mole) = 0.118 g.

It is lower than the mass of water in the flask (2.2 g).

3) For C₂H₅OH:

Pressure of C₂H₅OH at 308 K is 102.0 mmHg.

we need to convert from mmHg to atm: (1.0 atm = 760.0 mmHg).

P of C₂H₅OH = (1.0 atm x 102.0 mmHg) / (760.0 mmHg) = 0.13421 atm.

We must check if more 0.3 g of C₂H₅OH is evaporated,

n = PV/RT = (0.13421 atm) (3.0 L) / (0.082 L.atm/mol.K) (308 K) = 0.01594 mole.

m = n x molar mass = (0.01594 mole) (46.07 g/mole) = 0.7344 g.

It is more than the amount in the flask (0.3 g), so the pressure should be less than 0.13421 atm.

We have n = mass / molar mass = (0.30 g) / (46.07 g/mole) = 0.00651 mole.

So, P of C₂H₅OH = nRT / V = (0.00651 mole) (0.082 L.atm/mole.K) (308.0 K) / (3.0 L) = 0.055 atm.

So, total pressure = P of N₂ + P of H₂O + P of C₂H₅OH = 0.5 atm + 0.0553 atm + 0.055 atm = 0.6103 atm.

3 0

3 years ago