119g
From the volume of the flask, and the density of air under the conditions in the room, you can calculate the mass of air. The density of air varies with pressure, temperature, humidity, etc. At sea level and at 15 °C air has a density of approximately 0.001225 g/ml, so under these conditions, a liter flask would contain (1000 ml)(0.001225 g/ml) = 1.225 g of air.
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.
74.8 kPa.
If the weight of the flask and compound are 703.55 and the flask weighs 345.8, then the compound weighs 357.75 grams. Then the density in grams per milliliter is 1.59 g/mL (357.75 g / 225 mL). There are 1000 milliliters in one liter, so the density is also .00159 g/L.
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.
From the volume of the flask, and the density of air under the conditions in the room, you can calculate the mass of air. The density of air varies with pressure, temperature, humidity, etc. At sea level and at 15 °C air has a density of approximately 0.001225 g/ml, so under these conditions, a liter flask would contain (1000 ml)(0.001225 g/ml) = 1.225 g of air.
The density is lower.
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.
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.
If the weight of the flask and compound are 703.55 and the flask weighs 345.8, then the compound weighs 357.75 grams. Then the density in grams per milliliter is 1.59 g/mL (357.75 g / 225 mL). There are 1000 milliliters in one liter, so the density is also .00159 g/L.
An old instrument that works very well for solids and liquids is a pichnometer. It is a glass flask with a defined, exact volume and you determine the density by weighing the pichnometer full of water (known density at a specified temperature), the empty flask and the flask with a small amount of the solid or full of a liquid. Note: The liquid or solid should not dissolve in water. If the do, use a standard liquid of known density that will not dissolve the sample
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.
You can, but the volume will not be as accurate as using a graduated cylinder, and will probably give you an inaccurate density.