Kinetic Theory of Gases Questions and Answers

A steel rod is 3.00 cm in diameter at 25°C. A brass ring has an interior diameter of 2.992 cm at 25°. At what common temperature will the ring just slide onto the rod? (take, as = 11 x 10^-60C^-1, ab = 19 x 10^60C^-1)

z points Large helium-filled balloons are used to lift scientific equipment to high altitudes. What is the pressure in atm inside such a balloon if it starts out at sea level with a tempera of 11.610.0°C and rises to an altitude where its volume is twenty times the original volume and its temperature is -30.1°C ?

An ideal gas is taken through a cyclic thermo dynamical process through four steps. The amounts of heat involved in steps are Q₁ = 5960J, Q2 = -5585J, Q3 = -2980J, Q4 = 3645J ; respectively, the corresponding works involved are W₁ = 2200, W₂ = -825J, W3= -1100J and W4 respectively. Find the value of W4 and efficiency of the cycle A 1315 J, 10% B 765 J, 11% C both of them D none of these

0.517 moles of an ideal gas are confined to a rigid container (V = 6.1 L). The pressure of gas at T = 596 K was 5.11 atm. What is the pressure (in atm) at T = 1,375?

Ideal gases are often studied at standard ambient temperature and pressure (SATP). The International Union of Pure and Applied Chemistry (IUPAC) defines SATP to be T=25° C and P = 100 kPa.

What is the pressure of 350 m³ of a given gas containing 3.7 x 10^25 molecules held at a temperature of 85°C? (Use 1.38 x 10^-23 J/K for Boltzmann's Constant.) Round to the nearest whole Pascal of pressure. 257 Pa 523 Pa 1024 Pa 845 Pa

A rigid cylinder with a movable piston contains a sample of hydrogen gas. At 330. K, this sample has a pressure of 150. kPa and a volume of 3.50. L. What is the volume of this sample at STP? A)0.233 L B)1.96 L C)4.29 L D)6.26 L

A flask contains carbon monoxide and carbon dioxide gases. The partial pressures of each are 2235 psi and 1125 psi, respectively. What is the total pressure in the flask in psi?

According to the kinetic molecular theory, Particles present in matter are in constant rest. Matter possesses definite Internal energy. All collisions between particles are inelastic in nature. Matter has no mass but occupy a definite volume.

If the gas in a confined container (constant volume) were to have its temperature raised from 55 degrees C to 160 degrees C, what would the final gage pressure be if the initial pressure were 220 psig? Note: Temperature and pressure must be converted to their absolute values. This is a direct proportion. C° +273 = Kº PSIG + 14.7 = PSIA (A)295.13 psig (B)309.83 psig (C)166.65 psig

Pr4. An ideal gas is contained in a 8-L closed container at 20 degrees C. If the number of molecules in the gas is 15 x 1023 (one mole of gas contains 6.022 x 1023 molecules and 1 atm = 1.01 x 105 Pa, 1L-10^-3 m^3) a) What is the temperature in K and the volume in m^3 of the gas? b) How many moles of gas is in the container? c) What is the pressure of the gas in atm? d) If the pressure is increased to 10 atm, volume is kept constant and half of the molecules released what is the temperature of the gas in C?

3. Gas is contained in a 5.00-L vessel at a temperature of 23.0°C and a pressure of 5.00 atm. a) Determine the number of moles of gas in the vessel. b) How many molecules are in the vessel? If the volume is now reduced in half and pressure increased two times, what is the temperature in degree C now

One mole each of a diatomic gas and a monoatomic gas are brought to the same, very high temperature. What is the ratio of the diatomic gas' internal energy to the monoatomic gas' energy?

By using the expression for the pressure of the gas P = 1 3nmv², show that the average kinetic energy of a gas molecule is 3/2KT, where K is Boltzman's constant, T is temperature, n is the number of molecule per unit volume, m is the mass and v is the average speed of the molecule.

A fixed quantity of an ideal gas has a pressure, volume, and temperature given by P₁, V₁. and T₁. respectively. If the gas has its volume tripled and its temperature doubled, find its final pressure in terms of P₁.

Which of the following describes a situation that would violate the law of entropy? O an iron bar placed in a room becomes cooler than its surroundings Oiced tea and hot coffee left on a table reach the same temperature cold water taken from the refrigerator eventually reaches room temperature a metal pan heated on the stove cools off when removed from the burner

The threshold wavelength for ejection of electrons from a metal is 330 nm. The work function for the photoelectric emission from the metal is (h = 6.6 × 10−³4 Js) A. 1.2 × 10^-18 J B. 6.0 × 10-¹⁹ J C. 1.2 x 10^-20 J D. 6.0 × 10^-12 J

Suppose a gas-filled incandescent light bulb is manufactured so that the gas inside the bulb is at atmospheric pressure when the bulb has a temperature of 20°C. a) Find the pressure inside such a bulb when it is hot, assuming its average temperature is 60°C (an approximation) and neglecting any change in volume due to thermal expansion or gas leaks. What is the % increase in the pressure? (b) The actual final pressure for the light bulb will be less than calculated in part (a) because the glass bulb will expand. What will the actual final pressure be, taking this into account? What is the % increase in the pressure? Is this a negligible difference?

What is the average kinetic energy in joules of hydrogen atoms on the 5500 °C surface of the Sun? (b) What is the average kinetic energy of helium atoms in a region of the solar corona where the temperature is 6*10^5 K?