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At what pressure will the mean free path in room-temperature (20∘C)(20∘C) nitrogen be 1.3 mm ?
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- One of the chemical controversies of the nineteenth century concerned the element beryllium (Be). Berzelius originally claimed that beryllium was a trivalent element (forming Be3+ ions) and that it gave an oxide with the formula Be2O3. This resulted in a calculated atomic mass of 13.5 for beryllium. In formulating his periodic table, Mendeleev proposed that beryllium was divalent (forming Be2+ ions) and that it gave an oxide with the formula Be2O3. This assumption gives an atomic mass of 9.0. In 1894, A. Combes (Comptes Rendus 1894, p. 1221) reacted beryllium with the anion C5H7O2and measured the density of the gaseous product. Combess data for two different experiments are as follows: I II Mass 0.2022 g 0.2224 g Volume 22.6 cm3 26.0 cm3 Temperature 13C 17C Pressure 765.2 mm Hg 764.6 mm If beryllium is a divalent metal, the molecular formula of the product will be Be(C5H7O2)2; if it is trivalent, the formula will be Be(C5H7O2)3. Show how Combess data help to confirm that beryllium is a divalent metal.Calculate the kinetic energy of 53 moles of N2 at 262 °C. (R = 8.314 JK–1 mol–1)At what pressure will the mean free path in room-temperature (20∘C) nitrogen be 0.70 m
- Calculate ‘most probable velocity’ (Cmp) of oxygen at 40oC. (R= 8.314J/K/mol، 1J = 1Kgm2/s2)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.A mixture of CO2 and Kr weighs 37.6 g and exerts a pressure of 0.855 atm in its container. Since Kr is expensive, you wish to recover it from the mixture. After the CO2 is completely removed by absorption with NaOH(s), the pressure in the container is 0.293 atm. (a) How many grams of CO2 were originally present? (b) How many grams of Kr can you recover? (a) grams CO2: (b) grams Kr: 3. 8.
- A mixture of CO₂ and Kr weighs 29.6 g and exerts a pressure of 0.895 atm in its container. Since Kr is expensive, you wish to recover it from the mixture. After the CO₂ is completely removed by absorption with NaOH(s), the pressure in the container is 0.295 atm. (a) How many grams of CO₂ were originally present? (b) How many grams of Kr can you recover? (a) grams CO₂: g (b) grams Kr:Suppose you have 1.25 moles of gaseous napthalene (C10H8) at T = 292 K. What is the average kinetic energy of one molecule of napthalene? (The molar mass of napthalene is 128 g/mol. You may assume that the gas molecules behave ideally.)13) HgO (s) –→Hg (1) + O, (g)
- 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]Which of the following is true for the root-mean-square speed (urms) in m/s and the average translational kinetic energy (Ek) in J/molecule of NO2 (g) molecules at 15° C? Your answer: Urms : 395 Ek : 5.96 x 10-21 Urms : 12.5 Ek : 3.59 x 103 Urms : 395 Ek : 3.59 x 103 Urms : 39.3 Ek : 5.96 x 10-21 Urms : 12.5 Ek : 5.96 x 10-211) Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO2Cl2(g) ® SO2(g) + Cl2(g). This decomposition is endothermic. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00 liter bulb and the temperature is raised to 375K. (a) What would be the pressure in atmospheres in the bulb if no dissociation of the SO2Cl2(g) occurred? (b) When the system has come to equilibrium at 375K, the total pressure in the bulb is found to be 1.43 atmospheres. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium at 375K. Note: Please answer both A and B
