0
How can the amount of moles of a gas be related to the pressure volume and temperature of the sample?
Wiki User
∙ 9y ago
Depending on your experiment, the number of moles will or will not change. If the gas is in a sealed container, then obviously the number of moles does not change. But if the gas is in an open container, then the gas is free to move.
In this case, raising the temperature would cause the number of moles to go down. Because the temperature is going up, the pressure increases also. When the pressure goes up, the volume goes up, meaning the gas "wants" to spread out. In an unsealed container, the gas will leave and you will end up with less moles within the container.
Wiki User
∙ 15y ago
Wiki User
∙ 14y agoThe relationship between volume and moles can be shown by using the Ideal Gas Law:
The volume occupied by a gas at a specified temperature and pressure is directly proportional to the number of particles in a gas.
Formula: PV = nRT
Where P = pressure
V = volume in liters
T = temperature
n = the number of particles in moles
R = the gas constant, and depends on the units of pressure:
use 0.0821 if pressure is in atmospheres (atm),
use 62.4 if pressure is in millimeters of Mercury (mmHg),
or 8.31 if pressure is in kiloPascals (kPa).
Wiki User
∙ 7y agoYes, the number of moles (n) of a gas is related to the pressure (P), volume (V) and temperature (T), by the ideal gas law: PV = nRT
So, moles (n) = PV/RT (where R is the universal gas constant)
Wiki User
∙ 9y ago1 mole is equivalent to 22,414 L; and 1 mole has a number of molecules equal to the Avogadro number.
Wiki User
∙ 7y agoYou think probable to the relation: pV = nRT.
Wiki User
∙ 7y agoThis is the general law of gases: pV=nRt
Wiki User
∙ 10y agoIt goes up
Add your answer:
Earn +20 pts
If the temperature is increased What happens to the partial pressure of oxygen in a sample of air?
In a sample of air, an increase in temperature will result in an increase in the partial pressure of oxygen.
What happens to a fixed sample of gas when its temperature changes?
If a fixed sample of gas has a change of temperature pressure would increase.
What sample is highly compressible at high pressure and expandable at high temperature?
liquid
When a fixed sample of gas increases in volume what happens to the pressure and temperature?
The frequency of collisions is reduced
How are pressure and volume related in boyles law?
Boyle found that when the pressure of a gas at constant temperature is increased the volume of a gas decreases. P x V is a constant at constant Temperature Boyle's Law: P1V1 = P2V2
If the temperature is increased What happens to the partial pressure of oxygen in a sample of air?
In a sample of air, an increase in temperature will result in an increase in the partial pressure of oxygen.
What happens to a fixed sample of gas when its temperature changes?
If a fixed sample of gas has a change of temperature pressure would increase.
What sample of matter sublimes at room temperature and standard pressure?
cos2(s)
What sample is highly compressible at high pressure and expandable at high temperature?
liquid
Which term is defined as a measure of the average kinetic energy of particles in a sample?
temperature
The vapor pressure of a sample of boiling water is 380 torr The temperature of the water is?
The temperature of the water is 100 degrees celsius.
Which temperature change would cause the volume of a sample of an ideal gas to double when the pressure of the?
For the pressure to remain the same, the temperature would double if the volume also doubled.
What is A sample of gas occupies 1.55L at STP What will the volume be if the pressure is increased to 50 ATM while the temperature remains constant?
A sample of gas occupies 1.55L at STP. What will the volume be if the pressure is increased to 50 atm while the temperature remains constant?
If a fixed sample of a gas increases in temperature at a constant pressure its volume does what?
Increases in direct proportion to the increase in temperature (on an absolute scale).
What would cause the pressure in a sealed container of gas to increase?
temperature increase The pressure of a contained sample of gas can be increased by increasing its temperature, or by decreasing its volume, or by injecting additional mass into it.
How many moles of carbon dioxide are there in a 50.0 dm3 sample of the gas at a pressure of 100.0 kPa and a temperature of 50 degrees celsius?
See the Related Question (link to the left of this answer)."How many moles of carbon dioxide are there in a 50.0 dm3 sample of the gas at a pressure of 100.0 kPa and a temperature of 50 degrees celsius?" 1.86 moles
Is it possible to liquefy c02 at a temperature of 40 degrees celsius?
The critical temperature for carbon dioxide is 304K (87.8°F [31°C]). That means that no amount of pressure applied to a sample of carbon dioxide gas at or above 304K (87.8°F [31°C]) will cause the gas to liquefy. At or below that temperature, however, the gas can be liquefied provided sufficient pressure is applied. The corresponding critical pressure for carbon dioxide at 304K (87.8°F [31°C]) is 72.9 atmospheres (~73000 kPa). In other words, the application of a pressure of 72.9 atmospheres of pressure on a sample of carbon dioxide gas at 304K (87.8°F [31°C]) will cause the gas to liquefy. See related link to read more about the Liquefaction of Gases.
