Gas Laws

At which temperature and pressure will a sample of neon gas behave most like an ideal gas?

• 300. K and 2 atm

• 300. K and 4.0 atm

• 500. K and 2.0 atm

• 500. K and 4.0 atm

Which statement describes the particles of an ideal gas, based on the kinetic molecular theory?

• The volume of the particles is considered negligible.

• The force of attraction between the particles is strong.

• The particles are closely packed in a regular, repeating pattern.

• The particles are separated by small distances, relative to their size

The table below shows data for the temperature, pressure, and volume of four gas samples.

Which two gas samples contain the same number of molecules?

• I and II

• I and III

• II and III

• II and IV

Tags

NGSS.HS-PS3-2

Standard pressure is equal to

• 1 atm

• 1 kPa

• 273 atm

• 273 kPa

The concept of an ideal gas is used to explain

• the mass of a gas sample

• the behavior of a gas sample

• why some gases are monatomic

• why some gases are diatomic

A real gas behaves more like an ideal gas when the gas molecules are

• close and have strong attractive forces between them

• close and have weak attractive forces between them

• far apart and have strong attractive forces between them

• far apart and have weak attractive forces between them

A real gas differs from an ideal gas because the molecules of real gas have

• some volume and no attraction for each other

• some volume and some attraction for each other

• no volume and no attraction for each other

• no volume and some attraction for each other

Which of the following gases behaves most like an ideal gas?

• H₂(g)

• O₂(g)

• NH₃(g)

• CO₂(g)

At STP, which sample contains the same number of molecules as 3.0 liters of H₂(g)?

• 1.5 L of NH₃(g)

• 2.0 L of CO2(g)

• 3.0 L of CH4(g)

• 6.0 L of N2(g)

At the same temperature and pressure, 1.0 liter of CO(g) and 1.0 liter of CO₂(g) have

• equal masses and the same number of molecules

• different masses and a different number of molecules

• equal volumes and the same number of molecules

• different volumes and a different number of molecules