The previous exercise gives an expression for
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Physical Chemistry
- If relativistic effects were ignored, what temperature is required for hydrogen atoms to have an rms-average speed of 3.00 x 108 m/s? What do you think is the potential for actually achieving this temperature?arrow_forwardIf a liter of argon gas (Ar) is compared to a liter of neon gas (Ne), both at 75°C and two atmospheres of pressure, then: The Ne atoms are on the average moving more slowly than the Ar atoms. The average kinetic energy of the Ar atoms is greater than that of the Ne atoms. O The mass of one liter of Ar equals the mass of one liter of Ne. There are equal numbers of Ar and Ne atoms. The Ar and Ne atoms have the same average speed.arrow_forward✓ 1 ✓ 2 X 3 4 ✓ 5 6 7 ✓8 ✓9 10 11 12 13 A reaction at 13.0 °C evolves 337. mmol of dinitrogen difluoride gas. Calculate the volume of dinitrogen difluoride gas that is collected. You can assume the pressure in the room is exactly 1 atm. Be sure your answer has the correct number of significant digits. volume: I 10 5arrow_forward
- Describe in your own words the Kinetic Molecular Theory of gases. The Kinetic Molecular Theory of gases tells us that the energy content of any gas is related only to its temperature. It also tells us that it is possible to compute the "RMS" (root mean squared) velocity of any gas molecule if you know its formula weight and its temperature. Using this information describe how you might compute the RMS velocity of sulfur dioxide (SO2) in the atmosphere of the planet Venus (T = 820 F), the RMS velocity of oxygen (O2) in the atmosphere of Earth (T = 50 F), or the RMS velocity of carbon dioxide (CO2) in the atmosphere of Mars (T = - 80 F).arrow_forward3. A laser spectroscopist produces benzene clusters by seeding benzene within helium in a supersonic expansion. Benzene and helium molecules are mixed within a gas cylinder and stored in a lab at 22°C. What is the relative speed of the benzene and helium molecules within the cylinder?arrow_forward7. You are given two samples of gas at identical P, T, and V, all near room temperature. Gas A is monatomic and gas B is diatomic. Both gas A and gas B have the same molar mass. (a) In which gas do the particles have a greater speed? (b) In which gas do the particles have more kinetic energy? (c) The temperature of each gas is increased by 8. The particles in which gas now have a greater average speed? A greater change in internal energy?arrow_forward
- You are working in an oil refinery . Where you use hydrocarbon gases like methane ( CH4 ) , ethane ( C2H5 , and propane ( C3Hg ) and prepared a mixture . When measured the pressure at 25 ° C it turns out to be 7.50 am This gas mixture was then also used in a mass spectrophotometer and the following data was obtained Based on this information find the partial pressure of each gas and report respectively as their name .appeared in the questionarrow_forwardwhere m stands for the mass of the particle, v stands for the particle speed, T stands for the Temperature of the system, and k stands for the Boltzmann constant. What would be the relative average kinetic energies for the helium, neon, and argon at 100K? (think about what this would mean for each variable) Explain how you assigned the relative positions of each gas.arrow_forwardQ6. (a)The vander waals equation is used to describe the behaviour of real gases but still not so useful in many industrial applications. Explain why?(3) (b)In kinetic molecular theory of gases it is assumed that The molecules of the gases occupy negligible volume as compared to the total volume of the gas' which factor can be actually described by this postulate?(2)arrow_forward
- Helium occupies a volume of 3.8 L at –45°C. What was its initial temperature when it occupied 8.3 L? 568 cm3 of chlorine at 25°C will occupy what volume at -25°C while the pressure remains constant?arrow_forwardGay-Lussac's law of combining volumes states that the volumes of reactants and products are in small whole-number ratios. Which of the following is NOT an assumption for the law of combining volumes? All of these are assumed for the law of combining volumes. The products and reactants must all be at the same pressure. The products and reactants must all be gases. The products and reactants must all be at the same temperature.arrow_forwarddN F(V)dV = N M = 47(- `2 zRT" ,MV². 32v² exp(- 2RT AP(- Where dN, the number of particles having a velocity between v and v+dV, V velocity of molecules, M moleculer mass of gase, T temperature. = [v? fV)dV =?arrow_forward
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