CHEMISTRY-TEXT
8th Edition
ISBN: 9780134856230
Author: Robinson
Publisher: PEARSON
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Question
Chapter 10, Problem 10.95SP
Interpretation Introduction
Interpretation:
The average speed of nitrogen gas on hot day and cold day is to be calculated.
Concept introduction:
In accordance with the kinetic-gas theory the relation between average speed, temperature, and molar mass is as follows:
Where,
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Students have asked these similar questions
c) 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?
Explain the observations listed below using
the Kinetic Molecular Theory.
(a) When a balloon is placed into an
environment where its temperature goes
down, its volume decreases; this happens
regardless of the gas that is in the balloon.
(b) When the balloon which was just
described from above is cooled even further,
its volume doesn't become zero; instead, the
gas condenses or deposits out.
(c) If NH3 gas is injected at one end of a long
tube while HCI gas is injected simultaneously
at the other end, ammonium chloride forms
in the tube after a few minutes. The formation
is closer to the HCl end of the tube than the
NH3 end.
(d) A flag moves back and forth in the wind.
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/s
Chapter 10 Solutions
CHEMISTRY-TEXT
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