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3 years ago

Which of the following occupies a volume? solids liquids gases all of the above

Chemistry

2 answers:

sasho [114]3 years ago

5 0

<u>Answer:</u> The correct answer is all of the above.

<u>Explanation:</u>

Volume is defined as the amount of space that a substance is occupying. The S.I. unit of this property is Liter (L).

There are 3 states of matter:

Solid state: In this state, the particles of the state are orderly arranged and it occupies specific shape and volume.
Liquid state: In this state, the particles of the state are not orderly arranged and it occupies the shape and volume of the container.
Gaseous state: In this state, the particles are randomly arranged and the particles occupies the shape and volume of the container in which it is kept.

Hence, the volume is occupied by all the three states.

Thus, the correct answer is all of the above.

yanalaym [24]3 years ago

4 0

Solids, liquids and gases all take up volume.

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How many grams of Cl2 are in 1.20 x 1024 Cl atoms?

Vaselesa [24]

<h3>Answer:</h3>

70.906 g

<h3>Explanation:</h3>

We are given;

Atoms of Chlorine = 1.2 × 10^24 atoms

We are required to calculate the mass of Chlorine

We know that 1 mole of an element contains atoms equivalent to the Avogadro's number, 6.022 × 10^23.
That is , 1 mole of an element = 6.022 × 10^23 atoms

Therefore; 1 mole of Chlorine = 6.022 × 10^23 atoms

But since Chlorine gas is a molecule;

1 mole of Chlorine gas = 2 × 6.022 × 10^23 atoms

But, molar mass of Chlorine gas = 70.906 g/mol

Then;

70.906 g Of chlorine gas = 2 × 6.022 × 10^23 atoms

= 1.20 × 10^24 atoms

Thus;

For 1.2 × 10^24 atoms ;

= ( 70.906 g/mol × 1.2 × 10^24 atoms ) ÷ (1.20 × 10^24 atoms)

Therefore, 1.20 × 10^24 atoms of chlorine contains a mass of 70.906 g

5 0

3 years ago

Potassium is isotopic and has RAM of 39.5 work out the percentage abundance of each isotope in a given sample of potassium which

Troyanec [42]

Yo sup??

Let the percentage of K-39 be x

then the percentage of K-40 is 100-(x+0.01)

We know that the net weight should be 39.5. Therefore we can say

(39*x+40*(100-(x+0.01))+38*0.01)/100=39.5

(since we are taking it in percent)

39*x+40*(100-(x+0.01))+38*0.01=3950

39x+4000-40x-0.4+0.38=3950

2x=49.98

x=24.99

=25 (approx)

Therefore K-39 is 25% in nature and K-40 is 75% in nature.

Hope this helps.

3 0

3 years ago

(02.03 MC)

Olegator [25]

3 because of the thing it’s trying to say

7 0

3 years ago

C4H10 + 02 ➡️ H20 + CO2<br> balance the equation

Alexeev081 [22]

(Can I have Brainlist)?

Answer:

2C4H10 + 13O2 —> 8CO2 + 10H2O. Oxidation reaction

8 (4 moles CO2 per mole butane)

Explanation:

could be written C4H10 + 6 1/2 O2 —> 4CO2 + 5H2O

4 0

2 years ago

What are the mole fraction and the mass percent of a solution made by dissolving 0.21 g KBr in 0.355 L water? (d = 1.00 g/mL.) m

IRISSAK [1]

Answer:

Mol fraction H2O = 0.99991

Mol fraction KBr = 0.00009

mass % KBr = 0.059 %

mass % H2O = 99.941 %

Explanation:

Step 1: Data given

Mass of KBr = 0.21 grams

Molar mass KBr = 119 g/mol

Volume of water = 355 mL

Density of water = 1.00 g/mL

Molar mass water = 18.02 g/mol

Step 2: Calculate mass water

Mass water = 355 mL * 1g /mL

Mass water = 355 grams

Step 3: Calculate moles water

Moles water = mass water / molar mass water

Moles water = 355 grams / 18.02 g/mol

Moles water = 19.7 moles

Step 4: Calculate moles KBr

Moles KBr = 0.21 grams / 119 g/mol

Moles KBr = 0.00176 moles

Step 5: Calculate total moles

Total moles = 19.7 moles + 0.00176 moles

Total moles = 19.70176 moles

Step 6: Calculate mol fraction

Mol fraction H2O = 19.7 moles / 19.70176 moles

Mol fraction H2O = 0.99991

Step 7: Calculate mol fraction KBr

Mol fraction KBr = 0.00176 / 19.70176

Mol fraction KBr = 0.00009

Step 6: Calculate mass %

mass % KBR = (0.21 grams / (0.21 + 355) grams) *100%

mass % KBr = 0.059 %

mass % H2O = (355 grams / 355.21 grams) *100%

mass % H2O = 99.941 %

8 0

3 years ago