Total P ( in the flask) = Partial pressure(Ar) + Partial pressure (O2)
= [ n(Ar) +n(O2) ]*RT(final) / V(inal)
= [(1.2 * 0.6 / 0.0821*500)+( 501/760)*0.2/0.0821*400)]
*0.082 * 300 / 400/1000
= 1.33 atm
88.9237 moles
The gas pressure in the flask is lower than the atmospheric pressure when the water level is higher inside than outside the flask.
3.7 L
A properly prepared Dewar flask can contain liquid air, or any other liquid that needs shielding from ambient heat at standard temperature and pressure to avoid being evaporated.
A flask contains 0.410 of liquid bromine, . Determine the number of bromine molecules present in the flask.
At 30 degrees C, the vapor pressure of ethe is about 590 mm Hg. (The pressure requires 0.23 g of ether in the vapor phase at the fiven conditions, so there is sufficient ether in the flask.) At 0 degrees C, the vapo pressure is about 160 mm Hg, so some ether condenses when the tempeature declines.
To contain at 20 degrees celsius. To contain at 20 degrees Celsius. This would be written on a graduated cylinder or a volumetric flask.
88.9237 moles
1. When the flask was placed into the cold water, the colder air molecules in the flask move slower, putting out less pressure. With the decrease in air pressure inside the flask, the now greater pressure outside pushes water into the flask until the pressure inside equals the pressure outside.
The gas pressure in the flask is lower than the atmospheric pressure when the water level is higher inside than outside the flask.
0.77
I'm pretty sure NaOH is a solid under those conditions! You just need to know the density of NaOH. The temperature and pressure are irrelevant if it was a gas, you could use the Ideal Gas Law. See the Related Questions link to the left of this answer about that.
Yes
I the flask was sealed, the air inside of the flask would take up less space and as a result, cause a drop in pressure inside the flask.
74.8 kPa.
I'm guessing you are analyzing an experiment where you are determining the molecular mass of an organic liquid. You heated the flask and the liquid evaporated filling the flask, but escaping through a small hole in the covering. 1. Gases always fill the container. So, if the liquid evaporated and formed a gas (vapor), it filled the flask, 2. The pressure on the outside the flask is air pressure. since the vapor isn't pushing off the cover, the pressure is not higher than the air pressure. But since the extra escaped, it cannot be less than the air pressure. Therefore, it is the same.
See the Related Question to the left for how to solve Ideal Gas Law Problems so as to determine at what temperature to keep the flask so that the pressure is below the specified value.