Ideal Gas Laws and Assumptions

False (B)

273.15 K and 100 kPa

<p>low, high</p> Signup and view all the answers

<p>Pascal = Pa Atmosphere = atm Millimeters of mercury = mm Hg Bar = bar Pounds per square inch = psi</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>molar volume</p> Signup and view all the answers

<p>There are significant intermolecular forces between gas particles. (C)</p> Signup and view all the answers

<p>At low temperatures, the intermolecular forces become more significant compared to the kinetic energy of the molecules, causing deviations from the ideal gas behavior. High pressures lead to a reduction in the volume occupied by the gas molecules, making the assumption of negligible molecular volume less valid.</p> Signup and view all the answers

<p>Gas molecules are in continuous random motion = Assumption 1: Molecules of a gas are in constant random motion Collisions between molecules are perfectly elastic = Assumption 2: Collisions between molecules are perfectly elastic Intermolecular forces between gas particles are negligible = Assumption 3: There are no intermolecular forces between gas particles Kinetic energy is directly proportional to Kelvin temperature = Assumption 4: The kinetic energy of the molecules is directly proportional to Kelvin temperature Volume occupied by gas molecules is negligible = Assumption 5: The volume occupied by gas molecules is negligible compared to the volume of the container they occupy</p> Signup and view all the answers

<p>Real gases can condense into liquids at low temperatures, demonstrating that intermolecular forces are not negligible in real gases, unlike in the ideal gas model.</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>High temperature and low pressure (C)</p> Signup and view all the answers

At constant temperature, pressure is inversely proportional to volume.

The standard unit of pressure is Pascal (Pa), equivalent to N/m² or J/m³.

STP for gases is 273.15 K and 100 kPa.

Real gases deviate from ideal behavior at low temperature and high pressure.

Strong intermolecular forces reduce collisions, altering pressure-volume relationship.

A gas consisting of moving particles with negligible volume and no intermolecular forces.

Key assumptions include random motion, elastic collisions, negligible intermolecular forces, and proportional kinetic energy to temperature.

Collisions between gas molecules where no kinetic energy is lost.

The forces between gas particles are negligible compared to their kinetic energy.

The kinetic energy of gas molecules is directly proportional to the Kelvin temperature.

The volume occupied by one mole of an ideal gas at STP is a constant value.

The relationship described by PV = nRT, incorporating pressure, volume, temperature, and moles.

Real gases deviate from the ideal gas model at low temperatures and high pressures.