All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: The ideal gas law tends to become inaccurate when a. the pressure is lowered and molecular interactions become significant. b. the pressure is raised and the temperature is lowered. c. the temperature

Problem

The ideal gas law tends to become inaccurate when 

a. the pressure is lowered and molecular interactions become significant. 

b. the pressure is raised and the temperature is lowered. 

c. the temperature is raised above the temperature of STP.

d. large gas samples are involved.

e. the volume expands beyond the standard molar volume.


Solution

Among the 5 options, we´re asked to state which is the case when the Ideal Gas Law becomes inaccurate.


When dealing with the Ideal Gas Law:

PV=nRT

Where

P = pressure of the gas

V = volume of the gas

n = number of moles of gas

R = Ideal gas constant

T = temperature of the gas


But based on the Kinetic Molecular Theory, ideal gases are imaginary.


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