Dalton's Law of Partial Pressure Problems & Examples - Chemistry
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- čas přidán 26. 10. 2016
- This chemistry video tutorial explains the concept of dalton's law of partial pressure. It provides the equations plus plenty of examples and practice problems for you to work on.
Pressure & Boiling Point: • Introduction to Pressu...
Gas Pressure Unit Conversion:
• Gas Pressure Unit Conv...
Manometers & Barometers:
• Manometer Pressure Pro...
Water Height & Mercury Column:
• Height of Water in a B...
Boyle's Law Practice Problems:
• Boyle's Law Practice P...
_________________________________
How Does a Bike Pump Work?
• How Does a Bike Pump W...
Charles Law:
• Charles' Law
Gay Lussac's Law:
• Gay Lussac's Law Pract...
Avogadro's Law:
• Avogadro's law Practic...
Ideal Gas Law Problems:
• Ideal Gas Law Practice...
Combined Gas Law Problems:
• Combined Gas Law Problems
_______________________________
Gas Stoichiometry Problems:
• Gas Stoichiometry Prob...
Molar Mass of a Gas at STP:
• Molar Mass of a Gas at...
Gas Density at STP:
• Gas Density and Molar ...
Dalton's Law of Partial Pressure:
• Dalton's Law of Partia...
Collecting Gas Over Water:
• Collecting Gas Over Wa...
_______________________________
Gas Density of Mixtures:
• Gas Density & Average ...
Average Kinetic Energy of a Gas:
• Average Kinetic Energy...
Graham's Law of Effusion:
• Graham's Law of Effusion
Kinetic Molecular Theory of Gases:
• Kinetic Molecular Theo...
Gas Law Problems Review:
• Gas Law Problems Combi...
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that was easy to learn after some practice. I used to think it was really hard and i procrastinated learning partial pressures.
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If I keep a bucket of water which has vapour pressure of 2.34kPa @ 20°C, inside a closed room (ambient temp 20°C). It says water will keep evaporating until partial pressure is 2.34kPa for water vapour.
Does this mean that the total pressure of the room will increase?
Yes
Helpful for online classes
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In a gaseous mixture of CH4 and C2H6 there are twice as many moles of CH4 as C2H6. The partial pressure of CH4 is 40 mmHg. What is the partial pressure of C2H6?
what if 🤭🤧
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I have a question
what if thgases combined together
then check how it reacts and find it,s final mole after reacting for ex N2 +3H2 gives 2NH3 now let's suppose all n2 combined to give 5 mole of NH3 and there is still 3 mole of H2 left but only H2 will not react with NH3 so we can use dalton law now
What if we removed on substance from the mixture, what would be the effect of that and how can we write in an equation ?
For partial pressure, we take non reactive gases. Reaction between N2 & O2 is endothermic; so, partial pressure laws are applicable for them. I think if we remove one substance, the remaining others will occupy the total volume of container and will have partial pressure accordingly.
we don't have to divide it by the total?? 6:37
like 2 mol+3 mol. to get the total like the first example??
then divide each by the total like.. 2/5 and ,3/5??
if you divide it by the total then you're solving for the mole fraction
ur goated to the max
COULD YOU ANSWER THIS PROBLEM PLEASE?
A certain reaction occurs, producing an oxide of nitrogen as a gas. The gas has a
mass of 1.211 g and occupies a volume of 677 mL. The temperature in the laboratory is
23°C and the air pressure is 0.987 atm. Calculate the molar mass of the gas and
deduce its formula. Assume the gas is ideal.
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Why torr is used for unit in pressure?
3:55 the Xo2 or oxygen, where did the 10 came from? the denominator 10? how- where- what-
10 came from the total number of moles of the gases.
n(Ar) +n(O2) + n(N2)
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5 + 3 + 2 = 10
Sorry if i responded late!
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In the last sample problem, Is it possible to determine the number of moles of the CO2?
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in the pv=nrt formula, doesn't V have to be in metre cube? why did you substitute in the value which had litres ?
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If ideal gas equation is not applicable for any gas as they are real gases then why it is derived?????
Sir what if each gas is in a separate container and the mass ‘ temperature is given of individual gases but volume is not given
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just a little question isn't the universal gas constant 0.08314?
Hey in my textbook it says that the constant of R is 0.0821, is it the same or not?
0.08206 is more accurate, but 0.0821 works too. But, if you want a more accurate answer then stick with 0.08206 instead.
how to get the 0.08206..?
Lance Dela cruz You just plug it (0.08206 for R) into your equation. It is given to you, so you don’t need to find it.
Lance Dela cruz
PV=nRT
R=PV/nT
R=(1.0 atm)(22.4 L)/(1 mol)(273.15 K)
R=0.08206 (L•atm/mol•K)
The variables used were the conditions required to meet Standard Temperature and Pressure (STP).
0.08206 is a constant. Like Victor said, you just plug that number in.
Please can anyone help me abd tell me how get molar mass
molar mass is the equation drt/p (density*constant*temperature/ pressure) Hope that helps
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Partial Pressure 2:35
Since the question used 300K which is in Standard temperature, why did you 0.0821(R) instead of 8.315 in Standard pressure ?
I was wondering this too!
There are 2 of them, one for atm pressure which is (0.0821), and the other one is 8.315 which is the R for kPa. Its basically just difference in the units you use for your question. Sorry you probably know this by now because this is 3 months late lol.
@@danialbajwa8112 the question doesnt seem to specify a unit for pressure though, no?
R is a universal constant used in most chem problems, thus it does not change...u prolly know this by now
I thought the gas constant (R) was 8.314?
why do teachers make this concept so difficult?
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I need solution to this problem.
A sample of atmospheric air was found to contain 78% N2 , 0.03% of CO2, 16% O2, 1% rare gases,5% gaseous impurities at STP. If 200cm3 of the sample air was analyzed, calculate the volume of the respective component of the air hence calculate pressure 5 mole of the air will exert at STP.
how did you get 1000?
nvm just realized it
It's given in the question .
Total pressure 1000 turr
4:57
His voice is changed I think he was sick while recording this explanation :((
If h2 is collected over water at 22C and an atmospheric pressure of 100.8kPa, what is the partial pressure of the H2 when the water level inside the gas bottle is equal to the water level outside the bottle?
1:34 1:34
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can someone get back to me asap for the second formula how do u find R to be 0.08206
It's a constant
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where did he get 32g and 28g?
lmao idk if Im too late but he had gotten those measurements from the molar mass of the elements so the molar mass of oxygen is 16 but since the subscript is alway 2 when alone (2)16 is 32g. Same for the other elements
@@carolynwoo8483 yeah I look at the periodic table and I got it. still thankyouuu ^_^