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Thermal Properties of Matter MCQs for NEET — Physics Questions with Answers

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The Kelvin temperature scale is also known as the absolute scale of temperature. How is a temperature $t_C$ in Celsius related to its equivalent temperature T in Kelvin?

A. $T = t_C - 273.15$ B. $T = t_C + 273.15$ C. $T = 273.15 - t_C$ D. $T = t_C \times 273.15$

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Explanation

The THERMAL_PROPERTIES_OF_MATTER chapter states, 'temperature on these scales are related by T = $t_C$ + 273.15 (10.3)'. Lord Kelvin established this scale where 0 K is -273.15 Â°C.

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Which constant relates the pressure, volume, and absolute temperature for one mole of an ideal gas?

A. Boltzmann constant ($k_B$) B. Avogadro's number ($N_A$) C. Universal gas constant (R) D. Specific heat capacity (s)

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Explanation

The THERMODYNAMICS_Physics chapter states, 'An Equation of State (like the ideal gas equation PV = ÂµRT) is a relation connecting different state variables.' Here, R is the universal gas constant, and $\mu$ is the number of moles.

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For an ideal gas, the average kinetic energy of a molecule is proportional to which of the following?

A. Pressure of the gas. B. Volume of the gas. C. Absolute temperature of the gas. D. Nature of the ideal gas.

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Explanation

The KINETIC_THEORY chapter states, 'i.e., the average kinetic energy of a molecule is proportional to the absolute temperature of the gas; it is independent of pressure, volume or the nature of the ideal gas.' (Eq. 12.19, $E/N = 1/2 m\bar{v^2} = 3/2 k_B T$).

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The internal energy (E) of an ideal gas depends solely on which of the following thermodynamic variables?

A. Pressure and volume. B. Volume and temperature. C. Pressure and temperature. D. Temperature only.

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Explanation

The KINETIC_THEORY chapter states, 'Eq. (12.18) tells us that internal energy of an ideal gas depends only on temperature, not on pressure or volume.'

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In a mixture of non-interacting ideal gases, what is the total pressure?

A. The product of the partial pressures. B. The difference between the highest and lowest partial pressures. C. The sum of the partial pressures. D. The average of the partial pressures.

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Explanation

The KINETIC_THEORY chapter states, 'Thus, the total pressure of a mixture of ideal gases is the sum of partial pressures.' (Eq. 12.9: $P = P_1 + P_2 + \dots$).

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Which of the following is considered a state variable in thermodynamics?

A. Heat supplied ($\Delta Q$) B. Work done ($\Delta W$) C. Pressure (P) D. Path taken during a process

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Explanation

The THERMODYNAMICS_Physics chapter states, 'Examples of state variables are pressure (P), volume (V), temperature (T), and mass (m). Heat and work are not state variables.'

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If $P_1$, $V_1$, and $T_1$ represent the initial pressure, volume, and absolute temperature of a given sample of gas, and $P_2$, $V_2$, and $T_2$ represent its final state, which of the following relationships holds true for an ideal gas?

A. $\frac{P_1V_1}{T_1} = \frac{P_2T_2}{V_2}$ B. $\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$ C. $\frac{P_1T_1}{V_1} = \frac{P_2T_2}{V_2}$ D. $\frac{V_1T_1}{P_1} = \frac{V_2T_2}{P_2}$

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Explanation

The THERMAL_PROPERTIES_OF_MATTER chapter mentions, 'since PV = constant and V/T = constant for a given quantity of gas, then PV/T should also be a constant. This relationship is known as ideal gas law.' So, $\frac{PV}{T}$ is constant.

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The Boltzmann constant ($k_B$) serves as a link between which two physical domains?

A. Macroscopic thermodynamic variables and microscopic molecular quantities. B. Temperature and pressure. C. Volume and number of moles. D. Heat and work.

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Explanation

The KINETIC_THEORY chapter states, 'This is a fundamental result relating temperature, a macroscopic measurable parameter of a gas (a thermodynamic variable as it is called) to a molecular quantity, namely the average kinetic energy of a molecule. The two domains are connected by the Boltzmann constant.'

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For a constant volume gas thermometer, how is temperature read?

A. In terms of volume. B. In terms of pressure. C. In terms of heat supplied. D. In terms of density.

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Explanation

The THERMAL_PROPERTIES_OF_MATTER chapter states, 'Holding the volume of a gas constant, it gives P $\propto$ T. Thus, with a constant-volume gas thermometer, temperature is read in terms of pressure.'

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What is the universal gas constant R equal to, using the Boltzmann constant ($k_B$) and Avogadro's number ($N_A$)?

A. $R = k_B + N_A$ B. $R = k_B / N_A$ C. $R = N_A / k_B$ D. $R = k_B N_A$

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Explanation

The KINETIC_THEORY summary states, '$PV = \mu RT = k_B NT$ where N is the number of molecules. Since $N = \mu N_A$, then $R = k_B N_A$.

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