Evaluate the collision frequency of a 1:1 mixture of H2 anc 02 at 1.0 atm and 25 °C. Given the radius of H atom is 1.06 x 10-10 m and the radius of 0 atom is 9.6 x 10-11 m.
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- Calculate the collision frequency, z, and the collision density, ZAA, in carbon monoxide, d = 360 pm, at 30 °C and 120 kPa. What is the percentage increase when the temperature is raised by 10 K at constant volume?Given R= 8.31 J mol·' K-' mol', k= 1.38 x10-23 J K-', NA = 6.23 x 10²3 mol- 1. Calculate a) the mean translational kinetic energy of carbon dioxide molecule with a relative molecular mass of 44 at 20 °C [ans: 6.07×10-21 J] b) the mean translational kinetic energy of a molecule on an ideal gas at 10 °C? [ans: 5.86×10-21 J]Evaluate the collision frequency of a 1:1 mixture of H2 and 02 at 1.0 atm and 25 °C. Given the radius of H atom is 1.06 x 10-10 m and the radius of O atom is 9.6 x 10-11 m. |
- L Tab 14Collision theory depends on knowing the fraction of molecular collisions having at least the kinetic energy Ea along the line of flight. What is this fraction when (i) Ea = 15 kJ mol−1, (ii) Ea = 150 kJ mol−1 at (1) 300 K and (2) 800 K?A mixture of ideal gases having a total mass of 35 g is placed in a 13 L vessel at 269.0 K. The equilibrium pressure is measured to be 1.6 bar. Calculate the average molar mass of the gas mixture.Find the collision density (number of collisions / sec / m3) of NO with O3 at 300 K if the concentration at 1 atm total pressure are each 0.2 ppm (0.2 mg/L) and if the molecular diameters are 300 and 375 pm, respectively. The universal gas constant is given as 0.082 L atm K-1 mol-1. (Hint: For 1 ppm at 1 atm total pressure, the partial pressure is 1 x 10-6 atm)Use the kinetic theory to justify the following observations: (a) the rate of a reaction in the gas phase depends on the energy with which two molecules collide, which in turn depends on their speeds; (b) in the Earth’s atmosphere, light gases, such as H2 and He, are rare but heavier gases, such as O2, CO2, and N2, are abundant.Calculate the collision frequency, z, and the collision density, ZAA, in carbon monoxide, d = 360 pm, at 30°C and 120 kPa.5. Consider air (which consists of 79 mol% of N2 and 21 mol% of O2) at 300 K: (a) What is the self-collision rate of nitrogen molecules in number of collisions per m' per second? (b) What is the self-collision rate of oxygen molecules in number of collisions per m' per second? (c) What is the collision rate between oxygen and nitrogen molecules in number of collisions per m' per second? Hint: Use the hard-sphere model where all the collisions are effective. The diameters of oxygen molecules and nitrogen molecules are 3.61 Å and 3.75 Å, respectively. For self-collision scenarios, calculate reduced mass based on two molecules of the same size and mass and be mindful that the number of collisions is double counted.Calculate the collision frequency, z, and the collision density, ZAA, in ammonia, d = 380 pm, at 30 °C and 120 kPa. What is the percentage increase when the temperature is raised by 10 K at constant volume?Calculate the collision frequency for (a) a molecule in a sample of oxygen at 1.00 atm pressure and 25°C, and (b) a molecule of hydrogen in a region of interstellar space where the number density is 1.0 × 1010 molecules per cubic meter and the temperature is 30 K. Take the diameter of O2 to be 2.92 × 10-10 m and that of H2 to be 2.34 × 10-10 m.SEE MORE QUESTIONS