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States of Matter 1.12 Dalton-s Law of Partial Pressures Wiva k12 Chemistry Questions and Correct Answers (elaborations) with 100% Accurate , Verified , Latest fully Updated , 2024/2025 ,Already Passed , Graded A+, Complete solutions guarantee distinctio CA$11.60   Add to cart
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States of Matter 1.12 Dalton-s Law of Partial Pressures Wiva k12 Chemistry Questions and Correct Answers (elaborations) with 100% Accurate , Verified , Latest fully Updated , 2024/2025 ,Already Passed , Graded A+, Complete solutions guarantee distinctio
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States of Matter 1.12 Dalton-s Law of Partial Pressures Wiva k12 Chemistry Questions and Correct Answers (elaborations) with 100% Accurate , Verified , Latest fully Updated , 2024/2025 ,Already Passed , Graded A+, Complete solutions guarantee distinctions Rationales

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  • states of matter 112 dalton s law of partial pre
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States of Matter 1.12: Dalton's Law of Partial
Pressures Wiva k12 Chemistry
It is one thing to understand the behaviors of individual gases. But what happens when
the gas you are studying is actually a mixture of gases? Chemist John Dalton
considered this issue and formulated Dalton's law of partial pressures. In this lesson,
you will learn about Dalton's law of partial pressures and how it applies to chemistry,
mountain climbing, and scuba diving. - ✔✔The behavior of mixtures of gases can be
understood by using the law of partial pressures.

Although pure gases are used in many examples of the gas laws, many gases are
actually mixtures. For example, the air that we breathe is a mixture of 78% nitrogen,
21% oxygen, and 1% other gases (carbon dioxide, argon, hydrogen, and others). Do
mixtures of gases behave the same way as pure gases?

In 1801, John Dalton addressed the issue of gas mixtures. He found the following:
%

-Gas mixtures behave the same way that pure gases do.
-Individual gases behave independently of the mixture.
-Individual gases contribute to the pressure of the mixture.

Dalton's findings have important implications in scuba diving, flying aircraft at high
altitudes, mountain climbing, and chemistry. - ✔✔Dalton addressed the issue of gas
mixtures.

John Dalton develops the law of partial pressures.

Ptot=P1+P2... - ✔✔1801

The pressure of a gas is caused by the individual gas molecules colliding against the
walls of the container they are in. In a gas mixture at the same temperature, all
molecules of each gas have the same kinetic energy and collide with the same force.

, In a mixture of gases, each type of gas exerts pressure on the sides of the container.
Its contribution to the total pressure represents a partial amount of the total pressure.
The pressure exerted by one gas in a mixture of gases is called that gas's partial
pressure.

Dalton found that the total pressure of the gas mixture is equal to the sum of the partial
pressures of all the gases present. This is called Dalton's law of partial pressures. -
✔✔Dalton's law of partial pressures applies to mixtures of gases.

the pressure of one gas in a mixture of gases - ✔✔partial pressure

Scuba divers must also contend with the changes in pressure and the ways that those
changes affect the air in their lungs. At sea level, the air pressure is 100 kPa. As you
descend through the water, the pressure (exerted by water) increases by 100 kPa (1
atm) for every 10 m of depth. Your body transmits that water pressure freely to your
lungs. At 10 m deep, then, the pressure on the air in your lungs is 200 kPa. -
✔✔Scuba divers breathe air under pressure.
%

The increases in the partial pressures of nitrogen and oxygen in lungs cause problems
for divers. The increased partial pressure of nitrogen at depths drives nitrogen gas into
the diver's body tissues. The tissues and blood become saturated when the diver is
deep. If the diver ascends to the surface too quickly, then the rapid decrease in
nitrogen partial pressure (as water pressure lessens) causes the nitrogen to form
bubbles in the blood and tissues, similar to the way opening a bottle of soda causes it
to fizz. The bubbles can cause painful cramps and block blood flow to the heart and
brain, thereby producing decompression sickness, also called the bends. The bends
can be prevented by slow, controlled ascent, with the diver stopping for various times
at different depths to allow the nitrogen to come out of solution slowly without forming
bubbles. The times are available in dive tables or decompression tables. -
✔✔Increased nitrogen at depths is dangerous to divers.

In chemistry experiments, you will often collect a gas over water, with the gas bubbled
through water and collected in a tube (volume and pressure can be measured). But the
gas in the tube also contains some water vapor, so you must correct by using Dalton's
law:

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