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Nutka1998 [239]
3 years ago
11

Describe two tests that you can run to determine if something is a substance or a mixture.

Chemistry
1 answer:
ryzh [129]3 years ago
4 0

The difference between a substance and a mixture is that a substance is one of a kind, a material of the same composition throughout, on the contrary, a mixture is one or more different substances brought together and mixed together without changing the nature of each single substance.

One way to test it is to take two substances like sand and table salt. They should each be in granular form and in adequate amount to mix. Neither substance has changed after mixing the two. Even though it may not be easy or convenient to accomplish, each substance could be separated out from the mixture.

When it comes to two substances in lump form, it would not be a mixture when one lump is positioned next to the other lump because there are not enough pieces to combine.

However, there could be a mixture of three substances, like sand, table salt and graphite powder and there could be a mixture with four substances, etc., ad infinitum.

Mixtures are of solid substances in general. On the other hand, one starts referring to solutions when liquids are involved. Gases can be a mixture like for example, air is a mixture with nitrogen, oxygen, argon, etc.


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The smallest particle of an element that retains the chemical identity of that element is a/an
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Read 2 more answers
WHAT MASS OF 1,1 DICHLOROEHTANE MUST BE MIXED WITH 100G OF 1,1 DICHLOROTETRAFLUOROEHTANE TO GIVE A SOLUTION WITH VAPOR PRESSURE
vaieri [72.5K]

This is an incomplete question.

The complete question is:

1,1-dichlorotetrafluoroethane, CF3CCL2F, has a vapor pressure of 228 torr. What mass of 1,1-dichloroethane must be mixed with 100.0 g of 1,1-dichlorotetrafluoroethane to give a solution with vapor pressure 157 torr at 25 degrees celsius?

Answer: 46.9 g of 1,1 dichloroethane must be fixed with 100 g  of 1,1 dichlorotetrafluoroethane to give a solution with vapor pressure of 157 torr at 25^0C

Explanation:

As the relative lowering of vapor pressure is directly proportional to the amount of dissolved solute.

The formula for relative lowering of vapor pressure will be,

\frac{p^o-p_s}{p^o}=i\times x_2

where,

\frac{p^o-p_s}{p^o}= relative lowering in vapor pressure

i = Van'T Hoff factor = 1 (for non electrolytes)

x_2 = mole fraction of solute  

=\frac{\text {moles of solute}}{\text {total moles}}

Given : x g of solute is present in 100 g of solvent

moles of solute (1,1 DICHLOROEHTANE) = \frac{\text{Given mass}}{\text {Molar mass}}=\frac{xg}{98.96g/mol}moles

moles of solvent (1,1 DICHLOROTETRAFLUOROEHTANE ) = \frac{\text{Given mass}}{\text {Molar mass}}=\frac{100g}{170.92g/mol}=0.58moles

Total moles = moles of solute  + moles of solvent = \frac{xg}{98.96g/mol}+0.58

x_2 = mole fraction of solute   =\frac{\frac{xg}{98.96g/mol}}{\frac{xg}{98.96g/mol}+0.58}

\frac{228-157}{157}=1\times \frac{\frac{xg}{98.96g/mol}}{\frac{xg}{98.96g/mol}+0.58}

0.45=1\times \frac{\frac{xg}{98.96g/mol}}{\frac{xg}{98.96g/mol}+0.58}

x=46.9g

Thus 46.9 g of 1,1 dichloroethane must be fixed with 100 g  of 1,1 dichlorotetrafluoroethane to give a solution with vapor pressure of 157 torr at 25^0C

5 0
4 years ago
Liquid nitrogen is obtained from liquefied air and is used to prepare frozen goods and in low-temperature research. The density
Savatey [412]

Answer:

The density of the liquid is 808\ kg/m^3.

Explanation:

It is given that,

The density of liquid is 0.808 g/cm³

We need to convert the density into kg/m³

We know that,

1 kg = 1000 g

And 1 m = 100 cm

So,

d=0.808\ \dfrac{g}{cm^3}\\\\=0.808 \dfrac{(1/1000)\ kg}{(1//100\ cm)^3}\\\\d=808\ kg/m^3

So, the density of the liquid is 808\ kg/m^3.

4 0
4 years ago
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