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Dahasolnce [82]
3 years ago
5

Which example is NOT a model?

Chemistry
2 answers:
lidiya [134]3 years ago
7 0

Answer:

B

Explanation:

i think leter B it because

jeka57 [31]3 years ago
6 0
Plastic skeleton atom made of fruit
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What is the ph of 0.1 m naoh solution??
Rudik [331]
NaOH is a strong base so pH will be around 13 to 12. Whatever number of moles of NaOH you have approximately the pH of NaOH will be around 14 13 or 12  
7 0
3 years ago
Nature operates the same way everywhere in the universe except where we have evidence
babunello [35]

Answer:

true

Explanation:

5 0
3 years ago
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Last week you reacted magnesium with a hydrochloric acid aqueous solution and hydrogen gas was produced. Let's say that you coll
miv72 [106K]

Answer:

69.8 kilo Pasacl is the pressure of the hydrogen gas.

Explanation:

Mg+2HCl\rightarrow MgCl_2+H_2

Pressure at which hydrogen gas collected = p = 101.2 kilo Pascals

Vapor pressure water = p^o = 31.4 kilo Pascals

The pressure of hydrogen gas = P

The pressure at which gas was collected was sum of vapor pressure of water and hydrogen gas.

p=P+p^o

P =p-p^o=101.2 kPa-31.4 kPa=69.8 kPa

69.8 kilo Pasacl is the pressure of the hydrogen gas.

3 0
3 years ago
If a molecule can hydrogen bond, does it guarantee that it will have a higher boiling point than a molecule that cannot? Explain
saul85 [17]

Answer:

a): not necessarily due to London Dispersion Forces and dipole-dipole interactions.  

b): not necessarily due to London Dispersion Forces.

Explanation:

There are three major types of intermolecular interaction:

  • Hydrogen bonding between molecules with H-O, H-N, or H-F bonds and molecules with lone pairs.
  • Dipole-dipole interactions between all molecules.
  • London dispersion forces between all molecules.

The melting point of a substance is a result of all three forces, combined.

Note that the more electrons in each molecule, the stronger the London Dispersion Force. Generally, that means the more atoms in each molecule, the stronger the London dispersion force. The strength of London dispersion force between large molecules can be surprisingly strong.

For example, \rm H_2O (water) molecules are capable of hydrogen bonding. The melting point of \rm H_2O at \rm 1\; atm is around 0 \; ^{\circ}\rm C. That's considerably high when compared to other three-atom molecules.

In comparison, the higher alkane hexadecane (\rm C_{16}H_{34}, straight-chain) isn't capable of hydrogen bonding. However, under a similar pressure, hexadecane melts at around 18\; ^{\circ}\rm C above the melting point of water. The reason is that with such a large number of atoms (and hence electrons) per molecule, the London dispersion force between hexadecane molecules could well be stronger than that the hydrogen bonding between water molecules.

Similarly, the dipole moments in HCl (due to the highly-polar H-Cl bonds) are much stronger than those in hexadecane (due to the C-H bonds.) However, the boiling point of hexadecane under standard conditions is much higher (at around 287\; \rm ^\circ C than that of HCl.

3 0
3 years ago
How do forces between particles in gases compare to forces in the other
Ber [7]

Answer:

A. The forces in gases are weaker than forces in solids but stronger

than forces in liquids.

5 0
2 years ago
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