West Bengal Police Constable Special Mock Test

Chemistry - States of Matter

1 / 10

1) How does Henry's Law apply to the solubility of gases?

A) The solubility of a gas decreases with increasing pressure.

B) The solubility of a gas is independent of pressure.

C) The solubility of a gas increases with decreasing pressure.

D) The solubility of a gas increases with increasing pressure.

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2) How does the Van der Waals equation adjust for real gas behavior?

A) By keeping temperature constant.

B) By accounting for the volume occupied by gas molecules and intermolecular forces.

C) By ignoring intermolecular forces.

D) By assuming perfect elasticity of gas molecules.

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3) How does Dalton's Law relate to partial pressures in a gaseous mixture?

A) The total pressure is equal to the sum of the densities of the gases.

B) The total pressure is equal to the sum of the partial pressures of the gases.

C) The total pressure is determined by the gas with the highest partial pressure.

D) The total pressure is the average of the partial pressures of the gases.

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4) Which of the following statements best describes the difference in molecular motion between the three states of matter?

A) In gases, molecules are stationary compared to the vibrational movement in liquids and solids.

B) In solids, molecules vibrate in place while in liquids they slide past each other and in gases they move freely.

C) In solids, molecules move freely while in liquids and gases they vibrate in place.

D) In liquids, molecules are stationary, whereas in solids and gases they slide past each other.

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5) When a gas is compressed at constant temperature, why does its pressure increase according to kinetic molecular theory?

A) There is an increase in the average kinetic energy of molecules.

B) The volume of the gas increases.

C) The number of molecular collisions per unit area increases.

D) Molecules move faster when compressed.

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6) Which of the following best describes the triple point of a substance?

A) The temperature and pressure at which only solid and liquid phases coexist.

B) The temperature and pressure at which solid, liquid, and gas phases coexist in equilibrium.

C) The temperature and pressure at which only gas and liquid phases coexist.

D) The temperature and pressure at which only solid and gas phases coexist.

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7) Which property of gases can be explained by Avogadro's Law?

A) The density of a gas is proportional to its molar mass.

B) Volume changes with pressure.

C) Equal volumes of gases contain the same number of molecules at a given temperature and pressure.

D) Pressure changes with temperature.

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8) Consider a sealed container filled with ice. Upon heating, how does the transition from solid to liquid and then to gas illustrate energy changes in the system?

A) Energy is released during both melting and vaporization.

B) Energy is absorbed during both melting and vaporization.

C) Energy is released during melting and absorbed during vaporization.

D) Energy is absorbed during melting and released during vaporization.

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9) What characteristic is indicated by the compressibility factor of gases?

A) It indicates the boiling point of a gas.

B) It shows how incompressible a gas is.

C) It indicates how compressible a gas is compared to an ideal gas.

D) It reflects the solubility of a gas.

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10) Why do solids have definite shapes while liquids do not?

A) Solids have stronger intermolecular forces limiting molecular movement.

B) Solids are heavier than liquids.

C) Liquids are compressed more easily than solids.

D) Liquids have stronger intermolecular forces.

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Curriculum

Chemistry (States of Matter )

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