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Old Dalton's law of partial pressures states that in a gaseous mixture, the exerted by a component gas is the same as the pressure it would exert IF IT ALONE occupied the container.....
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In a mixture of oxygen and nitrogen gas, $80.0%$ of the total gas pressure is exerted by the nitrogen. If the total pressure is $"2.0 atm"$, what pressure does the oxygen exert?
$80%$of pressure is exerted by nitrogen gas. So, $20%$of pressure will be exerted by oxygen gas. $"p"_("O"_2) = 20% "of 2 atm" = 20/100 × "2 atm" = "0.4 atm"$
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A breathing mixture used by deep sea divers has a total pressure of 101.4 kPa and contains hellum, oxygen and carbon doxide. What is the partial pressure of oxygen if $P_(He) = 82.5 kPa$ and $P_(CO_2) = 0.4 kPa$?
And so $P_(O_2)=P_"Total"-P_(He)-P_(CO_2)$ $={101.4-82.5-0.4}*kPa$ $=18.5*kPa$ In commercial diving mixes I am not sure that carbon dioxide would be added in those quantities. I used to do a lot of recreational...
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A breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide What is the partial pressure of oxygen at $101.4$ $kPa$ if $P_(He)$ = $82.5$ $kPa$ and $P_(CO2)$ = $.4$ $kPa$?
The total pressure is the sum of the partial pressures of the given gases. $P_"Total"=P_"He"+P_"CO2"+P_"O2"$ Rearrange the equation to isolate $P_"O2"$, substitute the given values into the equation and solve....
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A vessel contains a mixture of nitrogen and oxygen. If the partial pressure of nitrogen is 20 atmospheres and the partial pressure of oxygen is 42.8 atmospheres, what is the total pressure inside the vessel?
Datlon's law of Partial Pressures states that in a gaseous mixture, the exerted by a gaseous component is the same as the pressure it would exert if it ALONE occupied...
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What is the partial pressure of helium gas in a sealed vessel that has a total pressure of 205 kPa and partial pressures of 15 kPa for chlorine and 89 kPa for fluorine?
Dalton's law of partial pressures states that in a gaseous mixture, the of a gaseous component is the same as the pressure that gas would exert if it ALONE occupied...
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What are the partial pressures exerted by each component exerted by a 4:1 mixture of oxygen and argon with respect to moles if the total pressure is $1*atm$?
$"Dalton's Law of partial pressures"$ states that in a gaseous mixture, the exerted by any component is the same the pressure it would exert if it alone occupied the container....
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A container of gas with a pressure of 450 kPa contains three different gasses -hydrogen, oxygen, and nitrogen. If the partial pressure of the hydrogen is 210 kPa and the partial pressure of the oxygen is 125 kPa, what is the partial pressure of nitrogen?
According to Dalton's law of partial pressures, the total pressure is equivalent to the sum of the pressures of the individual gases (if they were present alone). Therefore, the...
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A tank contains a mixture of helium, neon, and argon gases. lf the total pressure in the tank is 490. mmHg and the partial pressures of helium and argon are 21.5 mmHg and 10.2 mmHg, respectively, what is the partial pressure of neon?
And so... $P_"Total"=P_"He"+P_"Ne"+P_"Ar"=490*mm*Hg$ But we are given that $P_"He"=21.5*mm*Hg$, and that $P_"Ar"=10.2*mm*Hg$.. And so...$P_"Ne"={490-21.5-10.2}*mm*Hg}=458.3*mm*Hg$..
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A sample of hydrogen gas is collected over water at 25°C. The total pressure of the hydrogen and water vapor is 116.0 kPa. The partial pressure of water vapor at this temperature is 3.2 kPa. What is the pressure of the hydrogen gas alone?
This shouldn't feel too complicated... We know: what the vapor pressure of water vapor plus hydrogen gas is. what the vapor pressure of just water vapor is. Hence,...
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A mixture of $"N"_2$, $"O"_2$. and $"CO"_2$ has a total pressure of $"740 torr"$ In this mixture, the partial pressure of $"N"_2$ is $"120 torr"$ and the partial pressure of $"O"_2$ is $"400 torr"$. What is the partial pressure of $"CO"_2$ ?
From Dalton's Law of , the total pressure of a mixture of gases is the sum of the partial pressures of each gas. Therefore, the partial pressure of $"CO"_2$ is...
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