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When the water level is higher inside than outside the flask is the gas pressure in the flask higher than lower than or the same as the atmospheric pressure?
Yes
Assume you seal 1.0 g of diethyl ether in an evacuated 100 mL flask If the flask is held at 30 degrees Celsius what is the approx gas pressure 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.
Why was it necessary to match the water levels inside and outside the cooled flask before removing it from the water bath?
So to equalize the pressure inside the flask with that of the atmosphere.
Is the volume occupied by the gas in the flask approxmately the same greater or less than before it was heated?
Assuming the flask is sealed - the volume remains the same but the pressure increases
What is the pressure exerted by 1.55 g Xe gas at 20 C in a sealed 560 ml flask?
0,1013 MPa
Why did the water rush into the erlenmeyer flask when it was submerged in the cold water?
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.
When the water level is higher inside than outside the flask is the gas pressure in the flask higher or lower or the same as the atmospheric pressure?
The gas pressure in the flask is lower than the atmospheric pressure when the water level is higher inside than outside the flask.
When the water level is higher inside than outside the flask is the gas pressure in the flask higher than lower than or the same as the atmospheric pressure?
Yes
If you cool a flask to -200degrise what would happen to the air?
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.
A sample of nitrogen gas is stored in a 500.0ml flask at 108kpa and 10.0c the gas is transferred to a 750.0ml flask at 21.0c what is the pressure of nitrogen in the second flask?
74.8 kPa.
When all the liquid has evaporated the vapor totally fills the florence flask and exerts a pressure equal to the atmospheric pressure why?
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.
A flask with a capacity of 1.00dm contains 5.00g of ethane The flask will burst if the pressure exceeds 1.00x10 Pa at what temperature will the pressure of the gas exceed the bursting temperature?
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.
A gas held at 798 mmHg in a 400 mL flask is released into a 3 L flask What will be the new gas pressure?
106.4 mmHg
After 0.600 L of Ar at 1.20 ATM and 227 degrees celsius is mixed with 0.200 L of 0xygen gas at 501 torr and 127 celsius in a 400 ml flask at 27 celsius what is the pressure in the flask?
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
Assume you seal 1.0 g of diethyl ether in an evacuated 100 mL flask If the flask is held at 30 degrees Celsius what is the approx gas pressure 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.
How pressure capacity of glass flask is measured?
ASTM Standard C147-86
Why should you never heat a flask when sealed with a cork?
increased pressure and temperature
