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XI PHYSICS New Chapter 12 Kinetic Theory 222 Statement Pairs
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XI_PHYSICS_NEW CHAPTER_12_KINETIC THEORYXI_PHYSICS_NEW CHAPTER_12 KINETIC THEORY
11.1 INTRO; 12.2 MOLECULAR NATURE OF MATTER
S# False Statement True Statement
Atoms are made up of tiny particles that
1 Atoms consist of tiny particles that are in perpetual motion.
remain stationary.
Gases are composed of stationary atoms Gases consist of rapidly moving atoms with weak inter-
2
with strong inter-atomic forces. atomic forces.
Atoms attract each other when they are Atoms attract at a distance (e.g., van der Waals forces) but
3 close together, causing repulsion at a repel when too close. They attract when near, repel when
distance. squeezed.
The kinetic theory explains gas behavior by considering
The kinetic theory ignores inter-atomic
4 rapidly moving atoms with negligible inter-atomic forces, not
forces for gases.
ignoring them.
Kinetic theory cannot provide a molecular
Kinetic theory provides a molecular interpretation of gas
5 interpretation of pressure and
pressure and temperature, consistent with gas laws.
temperature.
Kinetic theory is essential for explaining specific heat
Kinetic theory has no relevance to specific
6 capacities of gases. Kinetic theory relates specific heat
heat capacities of gases.
capacities of gases to molecular parameters.
Kinetic theory estimates molecular sizes and masses from
Kinetic theory cannot estimate molecular
7 measurable gas properties, providing valuable insights into
sizes and masses from properties of gases.
molecular characteristics.
In gases, atoms are rigidly fixed in In gases, atoms are not rigidly fixed but are free to move. In
8
position. gases, atoms are not rigidly fixed; they can move freely.
Liquids consist of atoms or molecules that are in constant
Liquids consist of atoms that do not
9 motion. Liquids consist of atoms or molecules that are in
move.
motion.
In solids, atoms are closely packed with short interatomic
In solids, atoms have significant distances
10 distances. In solids, atoms are closely packed with short
between them.
interatomic distances.
In gases, the interatomic distances are much larger than
In gases, interatomic distances are in the
11 angstroms. In gases, interatomic distances are on the order
order of angstroms.
of tens of angstroms.
The mean free path in gases is extremely In gases, the mean free path is relatively long, enabling
12
short. molecules to travel significant distances without collisions.
Gases in dynamic equilibrium have
In dynamic equilibrium, gas molecules collide and change
13 constant properties without molecules
speeds constantly.
changing their speeds.
Atoms consist of only a nucleus and
Atoms have a nucleus containing protons and neutrons, in
14 electrons; no other subatomic particles
addition to electrons.
exist.
The kinetic theory is a complete and final The kinetic theory is a useful but not final explanation of
15
explanation of matter's nature. matter.
Protons and neutrons are indivisible
16 elementary particles with no Protons and neutrons are composed of quarks.
substructure.
Gas molecules have absolute freedom of
17 In gases, molecules collide frequently, leading to pressure.
motion and never collide with each other.
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, XI_PHYSICS_NEW CHAPTER_12_KINETIC THEORY
XI_PHYSICS_NEW CHAPTER_12 KINETIC THEORY
11.1 INTRO; 12.2 MOLECULAR NATURE OF MATTER
S# False Statement True Statement
The behavior of solids and liquids can be
18 accurately explained using the kinetic The kinetic theory mainly applies to gases.
theory designed for gases.
Gases consist of atoms that are stationary
19 In gases, atoms or molecules move rapidly and freely.
and never move.
The kinetic theory can provide insights
20 into the behavior of matter at the The kinetic theory primarily applies to macroscopic matter.
subatomic level.
The discovery of atoms and molecules
Discovery of atoms and molecules sparked further scientific
21 ended all scientific curiosity about
inquiry into matter.
matter's composition.
Atoms are the smallest and indivisible
Atoms consist of subatomic particles, including protons,
22 constituents of matter; nothing exists
neutrons, and electrons.
beyond them.
The concept of atoms was only introduced
Scholars in ancient India and Greece conjectured the
23 in modern science by John Dalton in the
existence of atoms well before John Dalton's atomic theory.
19th century.
In gases, atoms are tightly packed
In gases, atoms are widely spaced apart, unlike the closely
24 together, similar to how solids are
packed arrangement in solids.
arranged.
The kinetic theory of gases is based on the idea that gases
The kinetic theory explains gas behavior
25 consist of rapidly moving atoms or molecules, with negligible
by considering strong inter-atomic forces.
inter-atomic forces.
Gases are unable to flow because their
Gases can flow because their atoms or molecules are not
26 atoms are tightly fixed, similar to those in
rigidly fixed and can move around freely.
solids.
True atoms of elements do not possess physical attributes
Atoms of fire are smooth and round,
27 like being smooth, round, or thorny; such descriptions are
causing burns due to their thorny nature.
not scientifically accurate.
The kinetic theory primarily focuses on
The kinetic theory primarily explains the behavior of gases,
28 the behavior of solids and liquids due to
as short-range inter-atomic forces are negligible in gases.
their short-range inter-atomic forces.
Solid atoms move freely within solids,
Atoms in solids are relatively fixed in position, limiting their
29 allowing for their flow similar to that of
movement compared to atoms in liquids.
liquids.
The concept of atoms has always been The acceptance of the atomic theory faced skepticism and
30 universally accepted and never faced debate in the scientific community at various points in
skepticism in the scientific community. history.
All atoms consist of a nucleus and Atoms consist of a nucleus made up of protons and neutrons,
31 electrons and are not divisible into surrounded by electrons, and are further divisible into
smaller components. subatomic particles.
Quarks are the smallest and final
While quarks are among the subatomic particles, the search
32 constituents of matter, with no further
for the smallest elementary entities in matter continues
elementary entities.
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, XI_PHYSICS_NEW CHAPTER_12_KINETIC THEORY
XI_PHYSICS_NEW CHAPTER_12 KINETIC THEORY
12.3 BEHAVIOUR OF GASES
S# False Statement True Statement
The behavior of gases is easier to
The behavior of gases is easier to understand than that of
understand than that of solids and liquids
1 solids and liquids because gas molecules are far apart, with
because gas molecules are closer to each
negligible interactions except during collisions.
other, leading to stronger interactions.
The perfect gas equation, PV = RT, applies The perfect gas equation, PV = RT, applies to ideal gases
2 to all gases, including those that don't under specific conditions, and real gases may deviate from
follow ideal gas behavior. this behavior at high pressures and low temperatures.
Avogadro's hypothesis suggests that the
Avogadro's hypothesis states that the number of molecules
number of molecules per unit volume
3 per unit volume is the same for all gases at the same
varies for different gases at the same
temperature and pressure conditions.
temperature and pressure.
The number density (n) represents the
The number density (n) represents the number of molecules
4 number of molecules per unit volume and
per unit volume and is affected by temperature changes.
is not influenced by temperature.
An ideal gas is a theoretical model that approximates real
An ideal gas behaves exactly like a real
5 gases at low pressures and high temperatures but may not
gas at all pressures and temperatures.
precisely mimic real gas behavior under all conditions.
Boyle's law states that, at constant
Boyle's law states that, at constant temperature, the product
6 temperature, the volume of a gas is
of the volume and pressure of a gas is constant.
inversely proportional to its pressure.
Charles' law implies that, at constant
Charles' law implies that, at constant pressure, the volume of
7 pressure, the volume of a gas is directly
a gas is directly proportional to its absolute temperature.
proportional to its temperature.
Dalton's law of partial pressures is applicable to mixtures of
Dalton's law of partial pressures is not
8 ideal gases, where the total pressure is the sum of the partial
applicable to mixtures of ideal gases.
pressures of each gas.
The average distance between water The average distance between water molecules in the vapor
9 molecules in the vapor state is larger than state is significantly larger than in the liquid state due to the
in the liquid state. increased volume.
The molecular volume of water vapor is
The molecular volume of water vapor is significantly smaller
10 larger than the volume occupied by the
than the volume occupied by the water molecules.
water molecules.
The behavior of gases is more complex to
understand compared to solids and The behavior of gases is easier to understand than that of
11 liquids because gas molecules are in solids and liquids because gas molecules are in constant
constant equilibrium with no changes in motion, with dynamic equilibrium and changing properties.
their properties.
Atomic theory suggests that atoms are
Atomic theory suggests that atoms are not indivisible but
indivisible and elementary, consisting
12 consist of a nucleus (protons and neutrons) and electrons;
only of a nucleus and electrons, with no
even quarks may be part of substructures.
further substructures.
The ideal gas equation, PV = RT, remains
The ideal gas equation, PV = RT, applies to ideal gases under
consistent for all gases under any
13 specific conditions, and real gases may deviate from this
conditions, whether they are ideal or real
behavior at certain pressures and temperatures.
gases.
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