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Comparing the energy gaps of C (diamond), Si, and Ge, which statement is correct?
The NCERT states, 'For C (diamond), Si and Ge, the energy gaps are 5.4 eV, 1.1 eV and 0.7 eV, respectively.' This shows Ge has the smallest, then Si, then C.
What happens to electrons and holes when they gain external energy in a semiconductor?
The NCERT text mentions, 'Electrons rise up and holes fall down when they gain external energy.'
Which of the following equations correctly represents the ideal gas law?
According to the NCERT text (Chapter: THERMAL_PROPERTIES_OF_MATTER, Section 10.4; Chapter: KINETIC_THEORY, Summary point 1), the ideal gas equation relating pressure (P), volume (V), and absolute temperature (T) is given by PV = µRT, where µ is the number of moles and R is the universal gas constant.
The universal gas constant (R) has a value of approximately:
The NCERT text (Chapter: THERMAL_PROPERTIES_OF_MATTER, Section 10.4, and Chapter: KINETIC_THEORY, Summary point 1) states that the universal gas constant R = 8.31 J molâ»Â¹ Kâ»Â¹.
Real gases behave most like ideal gases under which of the following conditions?
The NCERT text (Chapter: KINETIC_THEORY, Section 12.3 and Summary point 1) mentions, 'Real gases satisfy the ideal gas equation only approximately, more so at low pressures and high temperatures.' Also, 'At low pressures or high temperatures the molecules are far apart and molecular interactions are negligible. Without interactions the gas behaves like an ideal one.'
If the temperature of a given mass of gas is kept constant, what can be inferred about the product of its pressure and volume (PV)?
According to Boyle's Law, derived from the ideal gas equation (PV = constant if µ and T are fixed), if temperature is constant, the product of pressure and volume remains constant (Chapter: KINETIC_THEORY, Section 12.3).
For a fixed pressure, the volume of a gas is directly proportional to its absolute temperature. This statement describes:
The NCERT text (Chapter: KINETIC_THEORY, Section 12.3) states, 'if you fix P, Eq. (12.1) shows that V ∠T i.e., for a fixed pressure, the volume of a gas is proportional to its absolute temperature T (Charles’ law).'
What is the relationship between the average kinetic energy of molecules and the absolute temperature of an ideal gas?
The NCERT text (Chapter: KINETIC_THEORY, Section 12.4.2) states, 'the average kinetic energy of a molecule is proportional to the absolute temperature of the gas [from E/N = (1/2)m <v^2> = (3/2)k_B T]'. This is a fundamental result.
For a mixture of non-interacting ideal gases, the total pressure is equal to:
The NCERT text (Chapter: KINETIC_THEORY, Section 12.3) mentions, 'the total pressure of a mixture of ideal gases is the sum of partial pressures.' This is also known as Dalton's Law of Partial Pressures.
The Boltzmann constant ($k_B$) is related to the universal gas constant (R) and Avogadro's number ($N_A$) by which of the following equations?
The NCERT text (Chapter: KINETIC_THEORY, Summary point 1) directly gives the relation: $k_B = R/N_A$.
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