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A 2.01-L sample of O2(g) was collected over water at a total pressure of 785 torr and 25°C. When the O2(g) was dried (water vapor removed), the gas has a volume of 1.92 L at 25°C and 785 torr. How would you calculate the vapor pressure of water at 25°C?
At constant number of mole $n$ and Temperature $T$, using the $PV=nRT$ we can write: $P_1V_1=P_2V_2$ We should calculate the pressure of pure $O_2$ in a $2.01L$ volume: $P_1=(P_2V_2)/V_1=(785" torr"xx1.92cancel(L))/(2.01cancel(L))=750"...
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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 mixture of oxygen, hydrogen, and nitrogen exerts a total pressure of 378 kPa. If the partial pressures of oxygen and hydrogen are 212 kPa and 101 kPa respectively, what is the partial pressure exerted by nitrogen?
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...
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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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Mixture containing .538mol $He$ gas, .315mol $Ne$ gas .103 $Ar$ gas, is confined in 7.00-L vessel at $25^o$Celsius. How do you calculate partial pressure of each gas in mixture? How would you calculate the total pressure of the mixture?
$"Dalton's law of partial pressures states that in a gaseous"$ $"partial pressure exerted by a component gas is the same as"$ $"the pressure it would exert if it alone occupied...
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If 5.0 of nitrogen gas and 5.0 g of chlorine gas are injected in to a 2.0 L vessel at a temperature of 65$"^o$C, what will the partial pressure of each gas be? What will the total pressure in the container be?
Dalton's law of holds that in a gaseous mixture the pressure exerted by a component gas is the same as if that gas ALONE occupied the container; the total pressure...
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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 container holds 6.4 moles of gas. Hydrogen gas makes up 25% of the total moles in the container if the total pressure is 1.24 atm. What is the partial pressure of hydrogen?
$P_"Total"=(n_"Total"RT)/V$ $=(n_(H_2)+n_"other gases")/V$ But $n_(H_2)=25%xxn_"Total"$. And thus $P_(H_2)=25%xxP_"Total"=25%xx1.24*atm=??$ For more spray, see This treatment relies on $"Dalton's Law of Partial Presssures"$, which states that in $"in a gaseous...
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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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