TS EAMCET Kinetic Theory of Gases — practice questions
112 free MCQs with worked solutions. Tap any question for the answer + explanation, or practice them all in the app.
Practice TS EAMCET Kinetic Theory of Gases in the app →The root-mean-square (rms) speed of gas molecules is given by:The mean translational kinetic energy of one molecule of an ideal gas at temperature $T$ is:If the absolute temperature of an ideal gas is doubled, the rms speed of its molecules:The mean free path $\lambda$ of a gas molecule of diameter $d$ at number density $n$ is approximately:For an ideal gas, the relationship between $C_p$ and $C_v$ is (Mayer's relation):The ideal gas equation is:The relation between universal gas constant $R$, Avogadro number $N_A$, and Boltzmann constant $k_B$ is:The **mean free path** of a gas molecule is:The pressure of an ideal gas in kinetic theory is given by:The **rms speed** of gas molecules at absolute temperature $T$ is:Average translational kinetic energy of a gas molecule at temperature $T$ is:The **law of equipartition of energy** states that, at temperature $T$, each quadratic degree of freedom contrNumber of degrees of freedom (DOF) of a monatomic gas (e.g. helium) molecule:Mayer's relation for an ideal gas is:**Adiabatic ratio** $\gamma$ of a gas is defined as:Number of degrees of freedom of a **rigid diatomic molecule** (e.g. O₂ at room temperature, vibrations not excIf vibrations are excited, a diatomic molecule has DOF:For a monatomic ideal gas, $C_V$ and $C_P$ per mole are:For a **rigid diatomic** ideal gas, $\gamma = C_P/C_V$ equals:The rms speed of N₂ at 300 K (M = 28 g/mol) is approximately (use $R = 8.314$ J/(mol·K)):If the temperature of a gas is doubled (at constant volume), the rms speed changes by a factor of:Average translational KE of a He atom at 300 K is approximately ($k_B = 1.38 \times 10^{-23}$ J/K):Mean free path of nitrogen at STP (d = 324 pm) is approximately:If P is doubled at constant T (compress gas isothermally), the mean free path:An ideal gas is held in a container at temperature T. The total internal energy of one mole of a monatomic gasFor a diatomic gas with all vibrational modes excited, the molar specific heat at constant volume is:The ratio of average KE of a monatomic gas to that of a rigid diatomic gas, at the **same T**, is:Velocity of sound in an ideal gas is $v_s = qrt{\gamma RT/M_0}$. Compared to rms speed, $v_s$:The rms speed of helium atom at 300 K is approximately (M_He = 4 g/mol):The internal energy of 2 moles of nitrogen gas (rigid diatomic) at 300 K is approximately ($R = 8.314$):If the mean free path of N₂ at 1 atm is ~80 nm, what is it at 0.01 atm (same T)?The number of moles of oxygen ($O_2$) gas in a vessel of volume 1 L at STP (273.15 K, 1.013 × 10⁵ Pa) is approIdeal gas equation:Postulate of kinetic theory: gas molecules:Avogadro's number:R / N_A =Root-mean-square speed of gas molecules (mass m):Average kinetic energy per molecule (monatomic gas):Degrees of freedom for monatomic gas (e.g., He, Ar):Most probable speed v_mp:Average speed v_avg of molecules:Maxwell speed distribution is:Internal energy of n moles of ideal gas (monatomic):Ratio of specific heats γ for monatomic gas:For ideal gas, C_p - C_v =Two gases of molar masses M₁ and M₂ at same T. Ratio of v_rms:Find v_rms of O₂ at 300 K (M = 32 g/mol, R = 8.314):Graham's law of effusion: rate of effusion ∝For Maxwell-Boltzmann distribution, fraction of molecules with KE > E behaves as:Boyle's law derivation from KTG: at constant T, doubling V causes:For monatomic ideal gas, U/T (heat capacity at const V) per mole:In adiabatic process for ideal gas:For mixture of two ideal gases, total pressure = (Dalton's law):Equipartition: at temperature T, each quadratic DOF carries energy:Mean free path doubles when:At what temperature does v_rms of H₂ equal v_rms of O₂ at 300 K?For diatomic gas at very high T (vibrational modes active), DOF = ?Boltzmann's distribution gives fraction of molecules in energy state E:During adiabatic compression of ideal gas:For an ideal gas in adiabatic process: TV^(γ-1) =Kinetic energy per molecule of monatomic gas at 300 K (k = 1.38 × 10⁻²³):Two containers, equal volume, one with H₂ and one with O₂ at same T, P. Ratio of:For ideal gas, molar heat capacity C_v vs C_p relationship:Speed of sound in ideal gas:Who discovered, in 1661, the gas law relating pressure and volume at fixed temperature?The kinetic theory of gases was mainly developed byWhich ancient Indian school of thought, founded by Kanada, gave a detailed atomic view of matter?In the Vaiseshika atomic theory, what was a molecule of two atoms called?John Dalton proposed his atomic theory mainly to explain which laws?By Gay Lussac's law, combining gas volumes areWhat is the approximate size of an atom?How does the force between two atoms behave with separation?How is the universal gas constant R related to the Boltzmann constant kB?Under which conditions does a real gas behave most like an ideal gas?A gas at 300 K is heated to 600 K at constant pressure. What happens to its volume?A gas occupies 6 L at 2 atm. It is squeezed to 3 L at constant temperature. New pressure?A mixture of 2 mol nitrogen and 3 mol argon has total pressure 10 atm. Partial pressure of nitrogen?Which law adds partial pressures to give a mixture's total pressure?Neon and oxygen in one vessel have partial pressures in the ratio 3:2. Ratio of their numbers of molecules?In the kinetic theory of an ideal gas, collisions of molecules are assumed to beA molecule of mass m and x-velocity vx rebounds elastically off a wall. Momentum change?Which expression gives the pressure of an ideal gas from kinetic theory?For an isotropic gas, the mean of vx² equals which fraction of the mean square speed <v²>?Hydrogen of density 0.09 kg/m³ has rms speed 1840 m/s. What pressure does it exert?What is the rms speed of nitrogen molecules at 300 K, approximately?At room temperature, molecular rms speeds in air are comparable toIf the absolute temperature of a gas becomes four times, its rms speedAt what temperature will O2 molecules have the same rms speed as H2 molecules at 300 K?A gas is at 27 °C. To what temperature must it be heated to double its rms speed?UF6 molecules with U-235 and U-238 have masses 349 u and 352 u. Ratio of their mean speeds?A gas's diffusion rate varies with molecular mass m asWhy does a gas warm up when a piston is pushed in to compress it?How many translational degrees of freedom does a molecule free to move in space have?Molecules of a monatomic gas such as argon have which degrees of freedom?A diatomic molecule treated as a rigid dumbbell has how many degrees of freedom in total?Under equipartition, one vibrational mode of a molecule contributes what average energy?What is the molar specific heat at constant pressure of helium treated as an ideal gas?What is the ratio of specific heats γ for a rigid diatomic ideal gas?A diatomic gas also has one active vibrational mode. What is its molar Cv?A polyatomic molecule has 3 translational, 3 rotational and f vibrational modes. Molar Cv?For any ideal gas, the difference Cp - Cv between molar specific heats equalsWhy do measured specific heats of Cl2 exceed rigid-model values?How much heat raises 1 mol of argon by 20 K at constant volume? (R = 8.31 J/mol K)Why does gas from a leak spread slowly through a room?Why do air molecules in a room not all settle on the floor under gravity?Where does a gas in equilibrium in a container exert pressure?Who proposed that equal gas volumes at equal T and P have equal molecule numbers?Who published Hydrodynamica in 1738, laying the basis for the kinetic theory of gases?Einstein (1905) and Smoluchowski (1906) supported kinetic theory with papers onWhich Roman philosopher, around 50 BC, said static bodies are made of rapidly moving atoms?Which physicist generalised Maxwell's velocity distribution in 1871?Kinetic theory assumes the total volume of the molecules themselves is