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madam [21]
3 years ago
8

Which is NOT a component of the kinetic theory of matter?

Chemistry
1 answer:
Vika [28.1K]3 years ago
5 0

Answer:

1) all matter is made up of atoms and molecules 2) these tiny particles are always in motion; the higher the temp. the faster they move 3) at the same temp., heavier particles move more slowly then small particles

Explanation:

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Calculate the molecular weights for NH3 and SF6.
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Hi there,

NH3 has the weight of 17.03 grams, and SF6 has the weight of 146.06 grams 

so in total, there is 163.09 grams

Hope this helps :P

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3 years ago
Which process(es) can be used to separate mixtures but not compounds?
hodyreva [135]
Think it would be distillation
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Most elements on the periodic table are
ivanzaharov [21]

Answer:

Metals

Explanation:

hope this helps

5 0
2 years ago
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Equation Given : Al^(3+) + Na3PO4 ==> 3Na^+ + AlPO4
Helga [31]

1 mols of Aluminium ion forms 1 mol aluminium phosphate

Molar mass of AlPO_4

  • 27+31+16(4)
  • 58+48
  • 106u

Moles of AlPO_4

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  • 0.000061/106
  • 5.75×10^{-7}
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Moles of Al3+=57.5µmol

3 0
2 years ago
A 1.25 g gas sample occupies 663 ml at 25∘ c and 1.00 atm. what is the molar mass of the gas?
lakkis [162]

Using ideal gas equation,  

P\times V=n\times R\times T

Here,  

P denotes pressure  

V denotes volume  

n denotes number of moles of gas  

R denotes gas constant  

T denotes temperature  

The values at STP will be:  

P=1 atm  

T=25 C+273 K =298.15K

V=663 ml=0.663L

R=0.0821 atm L mol ⁻¹

Mass of gas given=1.25 g g

Molar mass of gas given=?

Number of moles of gas, n= \frac{Given mass of the gas}{Molar mass of the gas}

Number of moles of gas, n= \frac{1.25}{Molar mass of the gas}

Putting all the values in the above equation,

1\times 0.663=\frac{1.25}{Molar mass of the gas}\times 0.0821\times 298.15

Molar mass of the gas=46.15

3 0
3 years ago
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