States of Matter

After some time, solid ammonium bromide appeared on the walls of the tube at point X.

Use the kinetic particle theory to explain this result.

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A gas syringe is filled with $70\text{ cm}^3$ of ammonia gas.
The pressure on the plunger is increased.
The temperature does not change but the volume in the syringe decreases to $60\text{ cm}^3$.

Use the kinetic particle theory to explain why the volume decreases.

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how the gases move through the tubes,

why the gases take different times to reach the litmus paper.

A gas syringe is filled with $80\text{ cm}^3$ of hydrogen chloride gas at $20\ ^\circ\text{C}$.
The syringe is placed in some hot water at $50\ ^\circ\text{C}$.
The atmospheric pressure does not change but the volume of the gas in the syringe increases to $88\text{ cm}^3$.

Use the kinetic particle theory to explain why the volume increases.

What is meant by the term evaporation?

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A sample of ethyl ethanoate in a beaker is moved into a colder room.

Explain, in terms of the kinetic particle theory, why this results in a decrease in the rate of evaporation.

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The table shows some information about different esters.

Which ester has the lowest rate of evaporation at room temperature and pressure?

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Explain your answer.

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What is meant by the term diffusion?

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What happens to the rate of diffusion of propyl ethanoate as the temperature of the room increases?

Explain your answer in terms of the kinetic particle theory.

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The table shows some information about different esters.

Which ester has the greatest rate of diffusion at room temperature and pressure?

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Explain your answer.

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Decene is a liquid at $25\text{ }^\circ\text{C}$.

How can you make this deduction from the data in the table?

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Butene boils at $-6\text{ }^\circ\text{C}$.

Use the kinetic particle theory to explain what happens when butene boils.

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A sample of ethene gas in a gas syringe is heated from $20\text{ }^\circ\text{C}$ to $100\text{ }^\circ\text{C}$.

The pressure remains constant.

Describe and explain, in terms of the kinetic particle theory, what happens to the volume of the gas.

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At room temperature ethene diffuses faster than butene.

Explain why.

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A sample of chlorine has a volume of $240\,\text{cm}^3$ at room temperature and pressure.

The pressure of the sample is increased at room temperature.

Describe and explain, in terms of kinetic particle theory, what happens to the volume of the sample.

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When heated at atmospheric pressure, iodine changes directly into a gas without becoming a liquid.

Describe the changes in particle separation, arrangement and motion during this change.

separation ______
arrangement ______
motion ______

At the same temperature and pressure, the rate of diffusion of chlorine gas is greater than that of iodine gas.

Explain why.

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A sample of oxygen has a volume of $540\,\text{cm}^3$ at room temperature and pressure.

The temperature of the sample is increased but the pressure is unchanged.

Describe and explain, in terms of kinetic particle theory, what happens to the volume of the sample.

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Sulfur is a gas above $445\,^\circ\text{C}$.

Describe the changes in particle separation, arrangement and motion when a sample of sulfur gas is cooled down to room temperature.

separation ______
arrangement ______
motion ______

Describe diffusion in terms of kinetic particle theory.

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Dodecane is a liquid at 25 °C.

How can you make this deduction from the data in the table?

Butane melts at –138 °C.

Use the kinetic particle theory to explain what happens when butane melts.

A sample of ethane gas at 0 °C is at a pressure of 1 atmosphere.

The pressure is increased but the temperature is maintained at 0 °C.

Describe and explain, in terms of the kinetic particle theory, what happens to the volume of the gas.

Draw a diagram to show the arrangement of the molecules in liquid bromine.
Show a bromine molecule as a circle.

A small amount of liquid bromine was placed in the bottom of a sealed flask. After thirty minutes the brown colour of the bromine had spread throughout the flask.

Use the kinetic particle theory to explain these observations.

Describe and explain how fractional distillation can be used to separate a mixture of neon, argon, krypton and xenon.

A mixture of neon, argon, krypton and xenon can also be separated by diffusion.

Explain why.

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