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Rina8888 [55]
3 years ago
7

An unknown substance was put in a container. The substance filled up the container from the bottom up, taking half of the space

in the container. What is most likely the state of matter of the substance?
Chemistry
1 answer:
ale4655 [162]3 years ago
6 0

Answer: The state of the substance is most likely to be is liquid state.

Explanation:

States of matter of three types:

1) Solids: In this state of matter particles are strongly associated due to high inter molecular forces acting between them. They have a fixed shape that is they doesn't take the shape of the container in which they are kept.

2) Liquids: In this state of matter particles are associated due to weak inter molecular forces acting between them. They don't have a fixed shape that is they take the shape of the container in which they are kept. They do not occupy the whole volume of the container.

3) Gases: In this state of matter particles are very weakly associated . They don't have a fixed shape that is they take the shape of the container in which they are kept. They occupy the whole volume of the container.

The state of the matter most likely is liquid state.

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Answer:

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6 0
3 years ago
A 0.652-g sample of a pure strontium halide reacts with excess sulfuric acid. the solid strontium sulfate formed is separated, d
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Answer:

The formula of the original halide is SrCl₂.

Explanation:

  • The balanced equation of this reaction is:

SrX₂ + H₂SO₄ → SrSO₄ + 2 HX, where X is the halide.

  • From the equation stichiometry, 1.0 mole of strontium halide will result in 1.0 mole of SrSO₄.
  • The number of moles of SrSO₄ <em>(n = mass/molar mass) </em>= (0.755 g) / (183.68 g/mole) = 4.11 x 10⁻³ mole.
  • The number of moles of SrX are  4.11 x 10⁻³ moles from the stichiometry of the balanced equation.
  • n = mass / molar mass, n =  4.11 x 10⁻³ moles and mass = 0.652 g.
  • The molar mass of SrX₂ = mass / n = (0.652) / (4.11 x 10⁻³ moles) = 158.62 g/mole.
  • The molar mass of SrX₂ (158.62 g/mole) = Atomic mass of Sr (87.62 g/mole) + (2 x Atomic mass of halide X).
  • The atomic mass of halide X = (158.62 g/mole) - (87.62 g/mole) / 2 = 71 / 2  g/mole = 35.5 g/mole.
  • This is the atomic mass of Cl.
  • <em>So, the formula of the original halide is SrCl₂</em>.
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