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Volume and pressure are held constant why does the hot air balloon rise and fall?
Wiki User
∙ 15y ago
Although volume and pressure are held constant, some of the gas escapes from the bottom of the balloon, thus decreasing the mass of the gas in the balloon. If mass is decreased, then density is also decreased because density=mass/volume. Such a decrease in density of the balloon causes it rise.
Wiki User
∙ 15y ago
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What are the effects of temperature and volume of gas samples at constant pressure?
If the volume is constant, the density does not change with temperature. With increasing temperature there is still the same number of molecules confined to the same volume of space, so no difference in density.
How does reducing the volume of gas affect its pressure if the temperature of the gas and the number of particles are constant?
The pressure is now higher.
What causes a balloon to fall to the ground?
It's very simple to see the answer. Balloons have a certain type of air pressure and because it is greater than the air around it, it climbs. However, when the air pressure in a balloon is less than the air pressure outside the balloon, the the balloon will start to descend.
What gas put in a balloon would make it fall?
Any gas that is more dense than air.Answer:It is a bit more complex than that - an air filled balloon would still fall because air has the density of air. In a normal inflated balloon the air in the balloon is compressed and has a density more than uncompressed air. If the "balloon" were a plastic bag wiith no air pressure above the pressure of the surrounding air, the balloon would still fall as the combined (average) density of the balloon/bag system is greater than the surrounding air. Even if the balloon were filled with a gas with a lower specific gravity than air the balloon wll fall if the compressed gas density excedes that of the surrounding air or if the combined (average) density of the balloon/bag or balloon system is greater than the surrounding air.
Choose the law that matches this definition As the temperature on a gas increases the volume of the gas must also increase to maintain constant pressure?
The concept of increased temperature calling for an increase in volume to maintain constant pressure can be found in the combined and/or ideal gas law. The combined gas law is PV=kNT, where P is pressure, V is volume, k is Boltzman's constant, N is number of gas molecules and T is temperature. The ideal gas law is PV=nRT where P is pressure, V is volume, n is number of moles of gas, R is gas constant and T is temperature. In both cases a rise in T would call for a rise in V to maintain constant P.
What are the effects of temperature and volume of gas samples at constant pressure?
If the volume is constant, the density does not change with temperature. With increasing temperature there is still the same number of molecules confined to the same volume of space, so no difference in density.
How does reducing the volume of gas affect its pressure if the temperature of the gas and the number of particles are constant?
The pressure is now higher.
What will change the size of the weather balloon as it rises?
The pressure of the air inside it. The higher the balloon rises, the lower the outside air-pressure. With less pressure outside, the balloon expands because of the pressure of the air inside it. Eventually, the balloon bursts, and scientists recover the instruments when they fall to earth.
What happens to a balloon after a cool change?
The drop in temperature will cause the atoms (or air) inside the balloon to fall in energy levels, this will result in the pressure inside the balloon dropping, and may cause the balloon to loose its shape.
What does Charles' Law state?
In thermodynamics and physical chemistry, Charles's lawis a gas law and specific instance of the ideal gas law, which states that:At constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its temperature (in Kelvin) increases or decreases.
Why mass and volume measurements for any sample of liquid should fall along the graph line?
mass and volume measurements for any sample liquid should fall along the graph line because liquids have a constant density. Density is mass over volume. Mass equals density which is a constant time volume.
Would a balloon rise in the absence of atmospheric pressure?
No. On the moon they just fall. (But it sure would expand !)
What causes a balloon to fall to the ground?
It's very simple to see the answer. Balloons have a certain type of air pressure and because it is greater than the air around it, it climbs. However, when the air pressure in a balloon is less than the air pressure outside the balloon, the the balloon will start to descend.
What would happen to pressure when the volume of gas was halved?
Boyles law states: P=c/V where P is pressure, c is some constant, and V is volume. It can more applicably express as PV=c by simple algebraic method. If C is to remain constant than anything that happens to P has to be undone by a reaction in V. So if P doubles, V has to fall by half.
What gas put in a balloon would make it fall?
Any gas that is more dense than air.Answer:It is a bit more complex than that - an air filled balloon would still fall because air has the density of air. In a normal inflated balloon the air in the balloon is compressed and has a density more than uncompressed air. If the "balloon" were a plastic bag wiith no air pressure above the pressure of the surrounding air, the balloon would still fall as the combined (average) density of the balloon/bag system is greater than the surrounding air. Even if the balloon were filled with a gas with a lower specific gravity than air the balloon wll fall if the compressed gas density excedes that of the surrounding air or if the combined (average) density of the balloon/bag or balloon system is greater than the surrounding air.
Choose the law that matches this definition As the temperature on a gas increases the volume of the gas must also increase to maintain constant pressure?
The concept of increased temperature calling for an increase in volume to maintain constant pressure can be found in the combined and/or ideal gas law. The combined gas law is PV=kNT, where P is pressure, V is volume, k is Boltzman's constant, N is number of gas molecules and T is temperature. The ideal gas law is PV=nRT where P is pressure, V is volume, n is number of moles of gas, R is gas constant and T is temperature. In both cases a rise in T would call for a rise in V to maintain constant P.
How would pressure be affected by an increase in the volume of the container?
All else being equal the pressure would fall
