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Propylene, C3H6, reacts with hydrogen under pressure to give propane, C3H8:
C3H6(g) + H2(g) -----> C3H8(g)
How many liters of hydrogen ( at 740 torr and 24 degree C) react with 18.0 g of propylene?
You would need $"11 L"$ of oxygen to react with that much propylene under those conditions for temperature and pressure. Start with the balanced chemical equation $C_3H_(6(g)) + H_(2(g))...
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A gas mixture consists of 0.4mole of N2, 0.6 mole of O2 and 0.2 mole of argon at a total pressure of 300kPa. Calculate the partial pressure of each gas in the mixture?
The idea here is that when you have a mixture of two or more gases, the of one component of that mixture will depend on how many moles said gas...
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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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A tank contains a mixture of 54.5 g of oxygen gas and 68.9 g of carbon dioxide gas at 38°C. The total pressure in the tank is 10.00 atm. How do you calculate the partial pressure (in atm) of each gas in the mixture?
You can solve this problem by using Dalton's Law of Partial Pressures, which states that the of a component of a gaseous mixture depends on the mole ratio of said...
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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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A mixture of two gases has a total pressure of 5.7 atm. If one gas has a partial pressure of 4.1 atm, what is the partial pressure of the other gas?
I got $"1.6 atm"$. DALTON'S LAW OF PARTIAL PRESSURES The equation that sums up what we have to do in this problem (pun intended) is Dalton's law of partial...
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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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A heliox deep-sea diving mixture contains 2.0 g of oxygen to every 98.0 g of helium. What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.2 atm?
And so we calculate the individual mole fractions.... $chi_(O_2)=((2.0*g*mol^-1)/(32.0*g*mol^-1))/{(2.0*g)/(32.0*g*mol^-1)+(98.0*g)/(4.0*g*mol^-1)}=2.54xx10^-3$ $chi_(He)=((98.0*g*mol^-1)/(4.0*g*mol^-1))/{(2.0*g)/(32.0*g*mol^-1)+(98.0*g)/(4.0*g*mol^-1)}=0.998$ And so $p_(O_2)=2.54xx10^-3xx8.2*atm=0.0208*atm$ The diver is at a serious depth....and had he or she been inhaling dinitrogen, i.e. from a...
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A mixture of $"N"_2$, $"O"_2$, and $"Ar"$ has mole fractions of $"N"_2 = .780$, $"O"_2 = .210$, and $"Ar" = .010$. What is the partial pressure of $"O"_2$ if the total pressure of the mixture is $"750 torr"$?
The idea here is that the partial pressures of the three gases will depend on the mole fraction each gas has in the mixture $->$ think Dalton's Law of Partial...
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A sample of carbon is placed in a rigid 1.50 L flask. Dinitrogen monoxide is added and the flask heated to 800C. When the system reached equilibrium the partial pressure of the carbon dioxide is found to be 0.030 atm and the partial pressure of the dinitrogen monoxide to be 1.48 atm. What is the partial pressure of nitrogen in the mixture.
The of nitrogen is 0.060 atm. First, write the balanced chemical equation for the equilibrium. C(s) +2N₂O(g) ⇌ CO₂(g) + 2N₂(g) There was no CO₂ or N₂ present at the...
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