General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
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Textbook Question
Chapter 9.6, Problem 9.18P
Calculate the average speed of a nitrogen molecule in m/s on a hot day in summer (T = 37 °C) and on a cold day in winter (T = −25 °C).
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Chapter 9 Solutions
General Chemistry: Atoms First
Ch. 9.1 - Yet another common measure of pressure is the unit...Ch. 9.1 - If the density of water is 1.00 g/mL and the...Ch. 9.1 - What is the pressure in atmospheres in a container...Ch. 9.1 - Prob. 9.4CPCh. 9.2 - Prob. 9.5CPCh. 9.3 - How many moles of methane gas, CH4, are in a...Ch. 9.3 - Prob. 9.7PCh. 9.3 - Prob. 9.8PCh. 9.3 - Prob. 9.9PCh. 9.3 - Prob. 9.10CP
Ch. 9.4 - Carbonate-bearing rocks like limestone (CaCO3)...Ch. 9.4 - Prob. 9.12PCh. 9.4 - Prob. 9.13PCh. 9.5 - What is the mole fraction of each component in a...Ch. 9.5 - What is the total pressure in atmospheres and what...Ch. 9.5 - Prob. 9.16PCh. 9.5 - Prob. 9.17CPCh. 9.6 - Calculate the average speed of a nitrogen molecule...Ch. 9.6 - At what temperature does the average speed of an...Ch. 9.7 - Prob. 9.20PCh. 9.7 - Prob. 9.21PCh. 9.8 - Assume that you have 0.500 mol of N2 in a volume...Ch. 9.9 - Prob. 9.23PCh. 9.9 - For ether, a partial pressure of 15 mm Hg results...Ch. 9.9 - Prob. 9.25PCh. 9 - Prob. 9.26CPCh. 9 - Prob. 9.27CPCh. 9 - Prob. 9.28CPCh. 9 - Prob. 9.29CPCh. 9 - Assume that you have a mixture of He (atomic...Ch. 9 - Prob. 9.31CPCh. 9 - Prob. 9.32CPCh. 9 - Prob. 9.33CPCh. 9 - Prob. 9.34CPCh. 9 - Prob. 9.36SPCh. 9 - Prob. 9.37SPCh. 9 - Prob. 9.38SPCh. 9 - Prob. 9.39SPCh. 9 - Prob. 9.40SPCh. 9 - Prob. 9.41SPCh. 9 - Assume that you have an open-end manometer filled...Ch. 9 - Assume that you have an open-end manometer filled...Ch. 9 - Prob. 9.44SPCh. 9 - Prob. 9.45SPCh. 9 - Prob. 9.46SPCh. 9 - Prob. 9.47SPCh. 9 - Prob. 9.48SPCh. 9 - Prob. 9.49SPCh. 9 - Prob. 9.50SPCh. 9 - Prob. 9.51SPCh. 9 - Prob. 9.52SPCh. 9 - Prob. 9.53SPCh. 9 - Prob. 9.54SPCh. 9 - Prob. 9.55SPCh. 9 - Prob. 9.56SPCh. 9 - Prob. 9.57SPCh. 9 - Prob. 9.58SPCh. 9 - Prob. 9.59SPCh. 9 - Prob. 9.60SPCh. 9 - Prob. 9.61SPCh. 9 - Prob. 9.62SPCh. 9 - Prob. 9.63SPCh. 9 - Prob. 9.64SPCh. 9 - Prob. 9.65SPCh. 9 - Prob. 9.66SPCh. 9 - Prob. 9.67SPCh. 9 - Prob. 9.68SPCh. 9 - Prob. 9.69SPCh. 9 - Prob. 9.70SPCh. 9 - Prob. 9.71SPCh. 9 - Prob. 9.72SPCh. 9 - Prob. 9.73SPCh. 9 - Prob. 9.74SPCh. 9 - Prob. 9.75SPCh. 9 - Prob. 9.76SPCh. 9 - Prob. 9.77SPCh. 9 - Prob. 9.78SPCh. 9 - Prob. 9.79SPCh. 9 - Prob. 9.80SPCh. 9 - Prob. 9.81SPCh. 9 - Prob. 9.82SPCh. 9 - Prob. 9.83SPCh. 9 - Prob. 9.84SPCh. 9 - Prob. 9.85SPCh. 9 - Prob. 9.86SPCh. 9 - Prob. 9.87SPCh. 9 - Prob. 9.88SPCh. 9 - Prob. 9.89SPCh. 9 - Prob. 9.90SPCh. 9 - Prob. 9.91SPCh. 9 - Prob. 9.92SPCh. 9 - Prob. 9.93SPCh. 9 - Prob. 9.94SPCh. 9 - Prob. 9.95SPCh. 9 - Prob. 9.96SPCh. 9 - Prob. 9.97SPCh. 9 - Prob. 9.98CHPCh. 9 - Prob. 9.99CHPCh. 9 - Prob. 9.100CHPCh. 9 - Prob. 9.101CHPCh. 9 - Prob. 9.102CHPCh. 9 - Prob. 9.103CHPCh. 9 - Prob. 9.104CHPCh. 9 - Prob. 9.105CHPCh. 9 - Prob. 9.106CHPCh. 9 - Prob. 9.107CHPCh. 9 - Prob. 9.108CHPCh. 9 - Prob. 9.109CHPCh. 9 - Prob. 9.110CHPCh. 9 - Prob. 9.111CHPCh. 9 - Prob. 9.112CHPCh. 9 - Prob. 9.113CHPCh. 9 - Prob. 9.114CHPCh. 9 - Prob. 9.115CHPCh. 9 - Prob. 9.116CHPCh. 9 - Prob. 9.117CHPCh. 9 - Prob. 9.118CHPCh. 9 - Prob. 9.119CHPCh. 9 - Prob. 9.120CHPCh. 9 - Prob. 9.121CHPCh. 9 - Prob. 9.122CHPCh. 9 - Prob. 9.123CHPCh. 9 - Prob. 9.124CHPCh. 9 - Prob. 9.125CHPCh. 9 - Prob. 9.126CHPCh. 9 - Prob. 9.127CHPCh. 9 - Prob. 9.128MPCh. 9 - Prob. 9.129MPCh. 9 - Prob. 9.130MPCh. 9 - The Rankine temperature scale used in engineering...Ch. 9 - Prob. 9.132MPCh. 9 - Combustion analysis of 0.1500 g of methyl...
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- The average kinetic energy of the molecules in a gas sample depends only on the temperature, T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed 3 RT rms speed V M where R = 8.314 J/(mol·K) and M is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (kg-m²/Is?). What is the rms speed of Cl, molecules at 365 K? rms speed: m/s What is the rms speed of He atoms at 365 K? rms speed: m/sarrow_forwardAt what pressure will the mean free path in room-temperature (20∘C)(20∘C) nitrogen be 1.3 mm ?arrow_forwardAt 298K, N2 molecules have a mean speed of 475 m/s. As a consequence, the probability to randomly pick 1 molecule at 475.00 m/s is extremely high. Select one: True Falsearrow_forward
- There are two particles, one is heavy and the other is light. The light particles diffuse faster than the heavy particles. This relationship is known as Graham’s Law of Effusion. Since both gases are at the same temperature, they must have the same average kinetic energy (½ mv2), where m is mass and v is the velocity (like speed). Since both gases have the same average kinetic energy, you can state that ½ mLvL2 = ½ mHvH2. Multiplying both sides by 2 gives you mLvL2 = mHvH2. Rearranging the equation to get both masses on the same side of the equation will give you mL/mH = VH2/VL2. In 3a and 3b, you probably noticed that the heavy gas particles took twice as long to diffuse as the light gas particles. This means that the light gas particles are moving twice as fast, VH/VL = ½. Therefore, VH2/VL2 = ¼. How many times heavier is the heavy gas compared to the light gas? If the light gas was Ne, what would be a reasonable identity for the heavy gas?arrow_forwardCalculate the most probable speed, the mean speed, and the mean relative speed of CO2 molecules at 20 °C.arrow_forwardWhich 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 10-21arrow_forward
- Calculate the average speed of oxygen (O2) molecules in a gas at T = 202 K, O2 atomic mass is 32 amu, where the atomic mass unit (amu) is 1.66 x 10-27 kg. Provide your answer in units of meters per second, but do not include the units in your answer, just the number in normal form to 3 significant digits.arrow_forwardEstimate the fraction of molecules at 100 °C with speeds less than 300 m>s.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_forward
- Helium gas is escaping from a spherical balloon at the rate of 2 cubic ft. per minute (2ft³/min). How fast is its surface area shrinking when the radius of the balloon is 12 ft?arrow_forwardMolecules of oxygen of the following isotopic composition are separated in an oxygen enrichment plant: 16O16O, 16O17O, 16O18O, 17O17O, 17O18O, 18O18O.(a) Compare the average translational kinetic energy of the lightest and heaviest molecular oxygen species at 200°C and at 400°C.(b) Compare the average speeds of the lightest and heaviest molecular oxygen species at the same two temperatures.arrow_forwardc) This relationship is known as Graham's Law of Effusion. Since both gases are at te same temperature, they must have the same average kinetic energy (½ mv²), where m is mass and v is velocity (like speed). Since both gases have the same average kinetic energy, you can state that ½ muvL2 = v ². Multiplying both sides by 2 gives you m v 2 y ². Rearranging the equation to get H H LL H H 2 m = m both masses on the same side of the equation will give you mu/mH = V 2/VL2. In 3a and 3b, you probably noticed that the heavy gas particles took twice as long to diffuse as the light gas particles. This means that the light gas particles are moving twice as fast, VH/VL = ½. Therefore, V 2/VL2 = ¼. How many times heavier is the heavy gas compared to the light gas? d) If the light gas was Ne, what would be a reasonable identity for the heavy gas?arrow_forward
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