Mention the different ways of increasing the number of molecular collisions per unit time in a gas. By reducing the volume of a gas at a constant temperature, the pressure of the gas increases. Explai

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Asked on May 14, 2026Physics

This physics problem tests your understanding of fundamental physical laws and their applications. The step-by-step solution below breaks down the problem using relevant equations and physical reasoning.

Accepted Answer · 2026-05-14T05:34:40.996Z

Here are the answers to your questions: 1) Mention the different ways of increasing the number of molecular collisions per unit time in a gas. Step 1: Identify factors affecting collision rate. The number of molecular collisions per unit time in a gas can be increased by: • Increasing the temperature: Higher temperature means molecules move faster, leading to more frequent collisions. • Decreasing the volume: Confining the same number of molecules to a smaller volume increases their density, resulting in more collisions with each other and the container walls. • Increasing the number of molecules: Adding more gas molecules to a fixed volume increases the density, thus increasing the collision frequency. The final answer is Increasing temperature, decreasing volume, or increasing the number of molecules. 2) By reducing the volume of a gas at a constant temperature, the pressure of the gas increases. Explain it on the basis of kinetic theory. Step 1: Relate pressure to molecular collisions. According to the kinetic theory of gases, the pressure exerted by a gas is due to the force of its molecules colliding with the walls of the container. Step 2: Explain the effect of reducing volume. When the volume of a gas is reduced at a constant temperature, the gas molecules are confined to a smaller space. This increases the number density of the molecules. Step 3: Conclude the effect on pressure. With more molecules per unit volume, the frequency of collisions between the molecules and the container walls increases. Since the temperature is constant, the average kinetic energy (and thus the average speed) of the molecules remains the same. Therefore, more frequent collisions with the same force per collision result in a greater total force per unit area, leading to an increase in pressure. The final answer is Reducing volume increases molecular density, leading to more frequent collisions with container walls, thus increasing pressure. 3) What do you mean by the root mean square speed of the molecules of a gas? Is the root mean square speed the same as the average speed? Step 1: Define root mean square speed. The root mean square (RMS) speed (v_rms) of gas molecules is a measure of the typical speed of particles in a gas. It is defined as the square root of the average of the squares of the speeds of all the individual molecules in the gas. v_rms = sqrt((v_1^2 + v_2^2 + + v_N^2)/(N)) Step 2: Compare RMS speed with average speed. No, the root mean square speed is not the same as the average speed. Because the speeds are squared before averaging, higher speeds contribute more significantly to the RMS value. Consequently, the RMS speed is always greater than or equal to the average speed for a distribution of speeds. The final answer is The root mean square speed is the square root of the average of the squared speeds; it is not the same as the average speed. 4) Why is the temperature below absolute zero not possible? Step 1: Define absolute zero. Absolute zero (0 K or -273.15^) is the theoretical lowest possible temperature at which particles in a substance possess the minimum possible kinetic energy. Step 2: Relate temperature to kinetic energy. Temperature is a direct measure of the average translational kinetic energy of the particles in a system. Step 3: Explain the impossibility. If a temperature below absolute zero were possible, it would imply that the particles have less than this minimum possible kinetic energy, which is physically impossible. It would mean they have negative kinetic energy, which is not allowed by the laws of physics. The final answer is Absolute zero represents the minimum possible kinetic energy of particles; going below it would imply impossible negative kinetic energy. 5) Estimate the average kinetic energy of a helium atom at the temperature on the surface of the sun (6000 K). Step 1: State the formula for average kinetic energy. The average translational kinetic energy (E_k) of an atom in an ideal gas is given by the formula: E_k = (3)/(2)kT where k is the Boltzmann constant (1.38 × 10^-23 J/K) and T is the absolute temperature in Kelvin. Step 2: Substitute the given values. Given temperature T = 6000 K. E_k = (3)/(2) × (1.38 × 10^-23 J/K) × (6000 K) Step 3: Calculate the average kinetic energy. E_k = 1.5 × 1.38 × 10^-23 × 6000 J E_k = 1.5 × 1.38 × 6 × 10^-20 J E_k = 12.42 × 10^-20 J E_k = 1.242 × 10^-19 J The final answer is 1.242 × 10^-19 J. 6) Show that the ratio of the root mean square speeds of molecules of two different gases at a certain temperature is equal to the square root of the inverse ratio of their masses. Step 1: State the formula for RMS speed. The root mean square speed (v_rms) of gas molecules is given by: v_rms = sqrt((3RT)/(M)) where R is the ideal gas constant, T is the absolute temperature, and M is the molar mass of the gas. Step 2: Write the RMS speeds for two different gases. For two different gases, Gas 1 and Gas 2, at the same temperature T: v_rms,1 = sqrt((3RT)/(M_1)) v_rms,2 = sqrt((3RT)/(M_2)) Step 3: Calculate the ratio of their RMS speeds. v_rms,1v_rms,2 = (sqrt(3RT)/(M_1))sqrt((3RT)/(M_2)) v_rms,1v_rms,2 = sqrt((3RT)/(M_1))(3RT)/(M_2) v_rms,1v_rms,2 = sqrt((3RT)/(M_1) × (M_2)/(3RT)) v_rms,1v_rms,2 = sqrt((M_2)/(M_1)) This shows that the ratio of the root mean square speeds is equal to the square root of the inverse ratio of their molar masses. The final answer is v_rms,1v_rms,2 = sqrt((M_2)/(M_1)). 7) Differentiate between the formations of white dwarfs and neutron stars. Step 1: Describe white dwarf formation. White dwarfs form from the remnants of low-to-medium mass stars (up to about 8 times the mass of our Sun) after they have exhausted their nuclear fuel. The star sheds its outer layers, leaving behind a dense core primarily composed of carbon and oxygen. This core is supported against gravitational collapse by electron degeneracy pressure. Step 2: Describe neutron star formation. Neutron stars form from the core collapse of much more massive stars (typically 8 to 20 times the mass of the Sun) after they undergo a supernova explosion. During the collapse, the immense gravitational forces overcome electron degeneracy pressure, forcing electrons and protons to combine into neutrons. The resulting extremely dense core is then supported by neutron degeneracy pressure. The final answer is White dwarfs form from low-mass stars supported by electron degeneracy, while neutron stars form from massive stars after supernovae, supported by neutron degeneracy. 8) Why do the gases at low temperatures and high pressure show large deviations from ideal behaviour? Step 1: Recall ideal gas assumptions. Ideal gases are theoretical gases that follow two main assumptions

Accepted Answer · 2026-05-14T05:34:40.996Z

Here are the answers to your questions: 1) Mention the different ways of increasing the number of molecular collisions per unit time in a gas. Step 1: Identify factors affecting collision rate. The number of molecular collisions per unit time in a gas can be increased by: • Increasing the temperature: Higher temperature means molecules move faster, leading to more frequent collisions. • Decreasing the volume: Confining the same number of molecules to a smaller volume increases their density, resulting in more collisions with each other and the container walls. • Increasing the number of molecules: Adding more gas molecules to a fixed volume increases the density, thus increasing the collision frequency. The final answer is Increasing temperature, decreasing volume, or increasing the number of molecules. 2) By reducing the volume of a gas at a constant temperature, the pressure of the gas increases. Explain it on the basis of kinetic theory. Step 1: Relate pressure to molecular collisions. According to the kinetic theory of gases, the pressure exerted by a gas is due to the force of its molecules colliding with the walls of the container. Step 2: Explain the effect of reducing volume. When the volume of a gas is reduced at a constant temperature, the gas molecules are confined to a smaller space. This increases the number density of the molecules. Step 3: Conclude the effect on pressure. With more molecules per unit volume, the frequency of collisions between the molecules and the container walls increases. Since the temperature is constant, the average kinetic energy (and thus the average speed) of the molecules remains the same. Therefore, more frequent collisions with the same force per collision result in a greater total force per unit area, leading to an increase in pressure. The final answer is Reducing volume increases molecular density, leading to more frequent collisions with container walls, thus increasing pressure. 3) What do you mean by the root mean square speed of the molecules of a gas? Is the root mean square speed the same as the average speed? Step 1: Define root mean square speed. The root mean square (RMS) speed (v_rms) of gas molecules is a measure of the typical speed of particles in a gas. It is defined as the square root of the average of the squares of the speeds of all the individual molecules in the gas. v_rms = sqrt((v_1^2 + v_2^2 + + v_N^2)/(N)) Step 2: Compare RMS speed with average speed. No, the root mean square speed is not the same as the average speed. Because the speeds are squared before averaging, higher speeds contribute more significantly to the RMS value. Consequently, the RMS speed is always greater than or equal to the average speed for a distribution of speeds. The final answer is The root mean square speed is the square root of the average of the squared speeds; it is not the same as the average speed. 4) Why is the temperature below absolute zero not possible? Step 1: Define absolute zero. Absolute zero (0 K or -273.15^) is the theoretical lowest possible temperature at which particles in a substance possess the minimum possible kinetic energy. Step 2: Relate temperature to kinetic energy. Temperature is a direct measure of the average translational kinetic energy of the particles in a system. Step 3: Explain the impossibility. If a temperature below absolute zero were possible, it would imply that the particles have less than this minimum possible kinetic energy, which is physically impossible. It would mean they have negative kinetic energy, which is not allowed by the laws of physics. The final answer is Absolute zero represents the minimum possible kinetic energy of particles; going below it would imply impossible negative kinetic energy. 5) Estimate the average kinetic energy of a helium atom at the temperature on the surface of the sun (6000 K). Step 1: State the formula for average kinetic energy. The average translational kinetic energy (E_k) of an atom in an ideal gas is given by the formula: E_k = (3)/(2)kT where k is the Boltzmann constant (1.38 × 10^-23 J/K) and T is the absolute temperature in Kelvin. Step 2: Substitute the given values. Given temperature T = 6000 K. E_k = (3)/(2) × (1.38 × 10^-23 J/K) × (6000 K) Step 3: Calculate the average kinetic energy. E_k = 1.5 × 1.38 × 10^-23 × 6000 J E_k = 1.5 × 1.38 × 6 × 10^-20 J E_k = 12.42 × 10^-20 J E_k = 1.242 × 10^-19 J The final answer is 1.242 × 10^-19 J. 6) Show that the ratio of the root mean square speeds of molecules of two different gases at a certain temperature is equal to the square root of the inverse ratio of their masses. Step 1: State the formula for RMS speed. The root mean square speed (v_rms) of gas molecules is given by: v_rms = sqrt((3RT)/(M)) where R is the ideal gas constant, T is the absolute temperature, and M is the molar mass of the gas. Step 2: Write the RMS speeds for two different gases. For two different gases, Gas 1 and Gas 2, at the same temperature T: v_rms,1 = sqrt((3RT)/(M_1)) v_rms,2 = sqrt((3RT)/(M_2)) Step 3: Calculate the ratio of their RMS speeds. v_rms,1v_rms,2 = (sqrt(3RT)/(M_1))sqrt((3RT)/(M_2)) v_rms,1v_rms,2 = sqrt((3RT)/(M_1))(3RT)/(M_2) v_rms,1v_rms,2 = sqrt((3RT)/(M_1) × (M_2)/(3RT)) v_rms,1v_rms,2 = sqrt((M_2)/(M_1)) This shows that the ratio of the root mean square speeds is equal to the square root of the inverse ratio of their molar masses. The final answer is v_rms,1v_rms,2 = sqrt((M_2)/(M_1)). 7) Differentiate between the formations of white dwarfs and neutron stars. Step 1: Describe white dwarf formation. White dwarfs form from the remnants of low-to-medium mass stars (up to about 8 times the mass of our Sun) after they have exhausted their nuclear fuel. The star sheds its outer layers, leaving behind a dense core primarily composed of carbon and oxygen. This core is supported against gravitational collapse by electron degeneracy pressure. Step 2: Describe neutron star formation. Neutron stars form from the core collapse of much more massive stars (typically 8 to 20 times the mass of the Sun) after they undergo a supernova explosion. During the collapse, the immense gravitational forces overcome electron degeneracy pressure, forcing electrons and protons to combine into neutrons. The resulting extremely dense core is then supported by neutron degeneracy pressure. The final answer is White dwarfs form from low-mass stars supported by electron degeneracy, while neutron stars form from massive stars after supernovae, supported by neutron degeneracy. 8) Why do the gases at low temperatures and high pressure show large deviations from ideal behaviour? Step 1: Recall ideal gas assumptions. Ideal gases are theoretical gases that follow two main assumptions

Mention the different ways of increasing the number of molecular collisions per unit time in a gas. By reducing the volume of a gas at a constant temperature, the pressure of the gas increases. Explai

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Mention the different ways of increasing the number of molecular collisions per unit time in a gas. By reducing the volume of a gas at a constant temperature, the pressure of the gas increases. Explai

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