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A gas mixture contains 1.19 g $N_2$ and 0.79 g $O_2$ in a 1.60-L container at 25 deg C. How do you calculate the mole fraction of $N_2$?
$chi_i=(n_i)/(n_"total")$. Now $n_"total"=(1.19*g)/(28.01*g*mol^-1)+(0.79*g)/(32.00*g*mol^-1)$ $=6.67xx10^-2*mol$ And $chi_"dinitrogen"$ $=$ $((1.19*g)/(28.01*g*mol^-1))/(6.67xx10^-2*mol)=0.64$. Given that it is a binary system, what is $chi_"dioxygen"?$ Note that the information given with respect to $"volume"$ and $"temperature"$...
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Five gases combined in a gas cylinder have the following partial pressures 3.00 atm ($N_2$), 1.80 atm ($O_2), 0.29 atm (Ar), 0.18 atm (He), and 0.10 atm (H). What is the total pressure that is exerted by the gases?
Old $"Dalton's Law of Partial Pressures"$ states that in a gaseous mixture, the exerted by a component gas is the same as it would have exerted if it alone occupied...
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What is the mole fraction of $NO$ in a 55.0 L gas cylinder at 30.0°C which comes from a mixture of $N_2$ and $NO$ if you have 3.238 mol of $N_2$ and the gas cylinder has a total pressure of 2.14 atm?
Your strategy here will be to use the equation in order to find the total number of moles present in the mixture, then use the number of moles of nitrogen...
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The atmospheric pressure at the summit of Mt. Everest is 255 torr. The percentage of $O_2$ and $N_2$ is 20% and 79%, respectively. How many $N_2$ and $O_2$ molecules are there in a volume of 10.0L at 12°C?
Your strategy here will be to use the equation to determine the total number of moles of air you have in that $"10.0-L"$ sample under those conditions for pressure and...
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When a container is filled with 3.00 moles of $H_2$, 2.00 moles of $O_2$, and 1.00 mole of $N_2$, the pressure in thecontainer is 768 kPa. What is the partial pressure of $O_2$?
Partial Pressure of $O_2$ = 256 kPa. Dalton's law of partial pressures covers two concepts; Mole fraction Partial pressure Let's talk about Mole Fraction first. You...
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If a mixture of gases with a total pressure of 1.0 atm contains 2 mol $He$, 4 mol $Ne$, and 2 mol $O_2$, what is the partial pressure of the $He$ in the mixture?
The of a gas that's part of a gaseous mixture will depend on two things the mole fraction said gas has in the mixture the total pressure of...
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What are the mole fractions of each component in a mixture of 15.08 g of $O_2$, 8.17 g of $N_2$, and 2.64 g of $H_2$? What is the partial pressure in atm of each component of this mix ture if it is held in a 15.50-L vessel at 15°C?
In order to be able to calculate the mole fraction of each component in the mixture, you will have to convert the masses given to you to moles. To...
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A tank contains $N_2$ at 1.0 atm and $O_2$ at 2.0 atm. Helium is added to this tank until the total pressure is 6.0 atm. What is the partial pressure of the helium?
In a gaseous mixture, the exerted by a gas is the same if that gas alone had occupied the container. The total pressure is the sum of the partial pressure....
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The composition of earths dry atmosphere is $78.8% N_2$, $21.0% O_2$, and $1.00% Ar$. Using the atospheric pressure recorded, which was 763 mm Hg with and an ambient temperature of 25 C, how do you calculate the partial pressures of these three gases?
And thus $P_"dinitrogen"$ $=$ $78.8%xx763*mm*Hg$. And $P_"dioxygen"$ $=$ $21.0%xx763*mm*Hg$.........etc. And the sum of the individual partial pressures is necessarily the overall pressure, $P=763*mm*Hg$
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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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