Question 1

Which state of matter has particles with the highest average kinetic energy?

Accepted Answer

Gas molecules move most rapidly and possess the highest average kinetic energy among the three common states of matter.

Question 2

At what temperature does water transition from liquid to gaseous state at standard atmospheric pressure?

Accepted Answer

Water boils at 100°C (373 K) at 1 atm pressure, marking the liquid-to-gas phase transition.

Question 3

What is the primary characteristic that distinguishes a liquid from a gas?

Accepted Answer

Liquids maintain a fixed volume due to stronger intermolecular forces, whereas gases expand to fill any container.

Question 4

Which of the following statements about the solid state is correct?

Accepted Answer

Solids possess a rigid crystalline structure with definite shape and volume due to strong intermolecular forces.

Question 5

What is the freezing point of water at standard atmospheric pressure?

Accepted Answer

Water freezes at 0°C (273 K) at 1 atm, marking the liquid-to-solid phase transition.

Question 6

At the triple point of water (611.7 Pa, 273.16 K), which statement is correct?

Accepted Answer

The triple point is the unique condition where solid, liquid, and gas phases of a substance coexist in thermodynamic equilibrium.

Question 7

A 500 mL sample of nitrogen gas at 27°C and 1 atm is heated to 327°C at constant volume. What is the final pressure?

Accepted Answer

Using Gay-Lussac's Law (P₁/T₁ = P₂/T₂): 1/300 = P₂/600; P₂ = 2.0 atm is incorrect; recalculating: 1/(27+273) = P₂/(327+273) gives P₂ = 2.0 atm—option C (2.5) represents 600K scenario.

Question 8

A gas at 2 atm pressure and 300 K occupies 10 L. If the gas is compressed isothermally to 5 atm, what is its final volume?

Accepted Answer

Using Boyle's Law (P₁V₁ = P₂V₂): 2 × 10 = 5 × V₂; V₂ = 4 L.

Question 9

At what temperature do water molecules have equal kinetic energy in all three states of matter (solid, liquid, gas)?

Accepted Answer

Kinetic energy differs across states at any given temperature; the triple point allows coexistence but not equal kinetic energies.

Question 10

The critical temperature of CO₂ is 31.1°C. What happens when CO₂ gas is compressed isothermally at 25°C?

Accepted Answer

Since 25°C < 31.1°C (critical temperature), isothermal compression causes CO₂ gas to liquefy.

Question 11

Which of the following correctly ranks the density of water in three states at standard conditions?

Accepted Answer

Water's liquid state (1 g/cm³) is denser than ice (0.92 g/cm³) due to hydrogen bonding patterns; gas is least dense.

Question 12

What is the defining characteristic that distinguishes the gaseous state from solid and liquid states?

Accepted Answer

Gases uniquely lack fixed shape and volume, expand to fill containers, and are highly compressible due to large intermolecular separations.

Question 13

Which phenomenon directly demonstrates that particles in a liquid state have sufficient kinetic energy to overcome surface tension effects?

Accepted Answer

Evaporation occurs when liquid molecules gain enough kinetic energy to escape the surface and transition to the gaseous state.

Question 14

A sample of dry ice (solid CO₂) at 195 K and 1 atm pressure is heated in a closed rigid container. If the temperature is raised to 310 K, what phase transition(s) will occur if the density of the system corresponds to a point above the critical density of CO₂ (critical density ≈ 467.6 kg/m³)?

Accepted Answer

At densities above critical density in a rigid container, heating solid CO₂ bypasses the liquid-gas boundary and transitions directly to a supercritical fluid above the critical point.

Question 15

The compressibility factor Z = PV/(nRT) for a real gas deviates from unity due to intermolecular forces. For a gas at low pressure and high temperature, which statement is most accurate regarding Z and molecular interactions?

Accepted Answer

At low pressure and high temperature, intermolecular distances are large, repulsive forces dominate over attractive forces, making Z > 1 and the gas approaches ideal behavior.

Question 16

At the critical point of a substance, the distinction between liquid and gas phases disappears. Which of the following correctly describes the critical temperature (Tc) and critical pressure (Pc) relationship for real gases using the van der Waals equation?

Accepted Answer

From van der Waals equation analysis at the critical point, Tc = 27a/(8Rb) and Pc = a/(27b²), where a and b are van der Waals constants.

CDS States of Matter

States of Matter — Practice Questions