28/03/2020 Kinetic Molecular Model of Matter and Temperature(Senior Class Physics Study by Topics) 28/03/2020 0Comments by Gate Academy Welcome to your Kinetic Molecular Model of Matter and Temperature(Senior Class Physics Study by Topics) NAME EMAIL PHONE NUMBER 1. Particules will experience large velocities at ... Low temperature High temperature Intermediate temperature None of the above 2. Under which conditions of temperature and pressure does oxygen gas behave most like an ideal gas High temperature and low pressure High temperature and high pressure Low temperature and high pressure Low temperature and low pressure 3. The kinetic molecular theory assumes that the particles of an ideal gas Are arranged in a regular geometric pattern Are in random, constant, straight-line motion Have collisions that result in the system losing energy Have strong attractive forces between them 4. The stoppers are removed from each container, which are in the same room at the same temperature. Which gas diffuses through the room the most slowly. Hydrogen Nitrogen Chlorine All at the same rate 5. Which statement is false The molecular weight of a gaseous compound is a non-variable quantity Gases can be expanded without limit. The density of a gas is constant as long as its temperature remains constant. (b) Pressure must be exerted on a sample of a gas in order to confine it. 6. The concept of an ideal gas is used to explain The behavior of a gas sample Why some gases are monatomic The mass of a gas sample Why some gases are diatomic 7. How do gas molecules move?: In curved-line paths In an orderly fashion Constantly and randomly In a circular motion 8. Under which conditions of temperature and pressure does a sample of neon behave most like an ideal gas? 400 K and 0.25 atm 100 K and 25 atm 400 K and 25 atm 100 K and 0.25 atm 9. What total gas volume (in liters) at 520oC and 880 torr would result from the decomposition of 33 g of potassium bicarbonate according to the equation:2KHCO3(s) K2CO3(s) + CO2(g) + H2O(g) 19 L 56 L 37 L 10 L 10. Calculate the weight of KClO3 that would be required to produce 29.5 L of oxygen measured at 127oC and 760 torr.2KClO3(s) 2KCl(s) + 3O2(g) 14.6 g 73.5 g 24.4 g 12.2 g 11. What is the kinetic energy of a 35 g of oxygen traveling at a velocity of 650 m/s? 7393.75 J 7393.75 KJ 7,393,750 J 7,393,750 KJ 12. Each of the containers is shown at the same temperature. In which container is the average speed of the particles the fastest? Oxygen Nitrogen Chlorine Hydrogen 13. Which postulate of KMT explains why gases are so easily compressed? 2- The particles of gas are in constant motion and move in straight lines. 3- The particles of gas do not exert any force of attraction or repulsion on each other. There is no energy loss during a collision. 4- The mean kinetic energy of the particles is directly proportional to their absolute temperature. 1‐ All particles are infinitely small and the size of a particle is negligible compared to the container that it holds. 14. Gases found in the environment are most likely to exhibit properties similar to that of ideal gases under conditions of: Low temperatures and high pressures Low temperatures and low pressures High temperatures and low pressures High temperatures and high pressures 15. The stopper is removed from the container of chlorine, at which temperature will the gas diffuse the fastest. 273 K 245 K 310 K 290 K 16. Gases are similar to liquids in that; They take the shape of their container They have a definite volume They cannot be compressed They are both considered fluids 17. The following states how gases differ from solids except; None of the above They have collisions with close neighbors They have a higher amount of kinetic energy They can be compressed 18. Which of the following changes requires an input of thermal energy? Freezing Deposition Evaporation Condensation 19. According to the kinetic molecular theory, which statement describes the particles in a sample of an ideal gas? The force of attraction between the gas particles is strong. The collisions between the gas particles cannot result in a transfer of energy between the particles. The motion of the gas particles is random and straight-line. The separation between the gas particles is smaller than the size of the gas particles themselves. 20. Which is defined as the combination of pressure and temperature at which all three states of matter can coexist at equilibrium? Melting point Critical point Deposition point Triple point 21. Which postulate of KMT explains why the scent of fresh coffee in the morning fills up every room in the house? 3‐ The particles of gas do not exert any force of attraction or repulsion on each other. There is no energy loss during a collision. 4‐ The mean kinetic energy of the particles is directly proportional to their absolute temperature. 1-All particles are infinitely small and the size of a particle is negligible compared to the container that it holds. 2‐ The particles of gas are in constant motion and move in straight lines. 22. Which is an intermolecular force? Covalent bond Metallic bond Ionic bond Hydrogen bond 23. The rate of HCl vs NH4 is Slower Equal Faster The same 24. Three 1.0 liter flasks are filled with H2, O2 and Ne, respectively, at STP.Which of the following statements is true? The velocity of the gas molecules is the same in each flask. Each flask has the same number of gas molecules. There are twice as many O2 and H2 molecules as Ne atoms. The density of each gas is the same. 25. A sample of nitrogen occupies 5.50 liters under a pressure of 900 torr at 25oC. At what temperature will it occupy 10.0 liters at the same pressure? -109°C 269°C 154°C 32°C 1 out of 25 Time is Up! Time's up
