At standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (d) Are the molar volumes in the solid state as similar as they are in the gaseous state?

Verified step by step guidance

Understand that the molar volume of a gas at standard temperature and pressure (STP) is approximately 22.4 L/mol, which is close to the given values for Cl2 and NH3 gases.

Recognize that gases have similar molar volumes at STP due to the ideal gas law, which states that one mole of any ideal gas occupies the same volume under the same conditions of temperature and pressure.

Consider the properties of solids: In the solid state, molecules are closely packed, and the molar volume is determined by the size and arrangement of the molecules, which can vary significantly between different substances.

Acknowledge that Cl2 and NH3 have different molecular structures and intermolecular forces, leading to different packing efficiencies and molar volumes in the solid state.

Conclude that the molar volumes of Cl2 and NH3 in the solid state are likely to be less similar than in the gaseous state due to differences in molecular structure and intermolecular interactions.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molar Volume

Molar volume is the volume occupied by one mole of a substance at a given temperature and pressure, typically measured in liters per mole (L/mol). At standard temperature and pressure (STP), the molar volume of an ideal gas is approximately 22.4 L/mol. This concept is crucial for comparing the behavior of gases and understanding how their volumes change under different states of matter.

States of Matter

Matter exists in different states, primarily solid, liquid, and gas, each with distinct properties. In solids, particles are closely packed and vibrate in fixed positions, leading to a much lower molar volume compared to gases, where particles are far apart and move freely. Understanding these states helps in analyzing how substances behave under varying conditions, such as temperature and pressure.

Comparative Analysis of Gases and Solids

When comparing the molar volumes of gases and solids, it is essential to recognize that gases typically have much larger molar volumes due to the significant space between particles. In contrast, solids have tightly packed particles, resulting in much smaller molar volumes. This difference highlights the impact of intermolecular forces and particle arrangement on the physical properties of substances in different states.

Recommended video:

Guided course

06:11

Dimensional Analysis

Related Practice

Textbook Question

At room temperature, Si is a solid, CCl₄ is a liquid, and Ar is a gas. List these substances in order of (a) increasing intermolecular energy of attraction

views

Textbook Question

At standard temperature and pressure, the molar volumes of Cl₂ and NH₃ gases are 22.06 and 22.40 L, respectively (b) On cooling to 160 K, both substances form crystalline solids. Do you expect the molar volumes to decrease or increase on cooling the gases to 160 K?

Textbook Question

At standard temperature and pressure, the molar volumes of Cl₂ and NH₃ gases are 22.06 and 22.40 L, respectively. (c) The densities of crystalline Cl₂ and NH₃ at 160 K are 2.02 and 0.84 g/cm³, respectively. Calculate their molar volumes.

Textbook Question

Benzoic acid, C₆H₅COOH, melts at 122 °C. The density in the liquid state at 130 °C is 1.08 g/cm³. The density of solid benzoic acid at 15 °C is 1.266 g/cm³. (b) If you converted a cubic centimeter of liquid benzoic acid into a solid, would the solid take up more, or less, volume than the original cubic centimeter of liquid?

views

Textbook Question

(a) Which type of intermolecular attractive force operates between all molecules?

views

Textbook Question

(b) Which type of intermolecular attractive force operates only between polar molecules?

views