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1 bar is 100,000 pascals.
I'm assuming you're working from a near-vacuum and initially at room temp.
Also, I'm using what's called the ideal-gas equation. It is an approximation that works best for gasses at low pressures and high temperatures. The equation is:
pV=nRT
p is pressure (in pascals)
V is volume (in meters cubed)
n is the amount of a substance (in moles)
R is a constant, 8.3145J/mol*K
T is temperature (in Kelvin. room temperature is kelvin is about 295)
If we try to solve for n now, we won't get it. We have another variable we need to take care of, T. So we...
Use this other equation:
(PV)/T of the initial state equals (pV)/T of the final state:
p1*V1/T1=p2*V2/T2
solve to T2:
T2=(p2*V2*T1)/(p1*V1)
Plug in values:
T2=(100,000Pa*.000032865m^3*295K)/(1pa*.000032865m^3)
which is saying that your new temp is 295000K (which is, like 600,000ºF)
And that's where I thought about quiting.
But no:
I plugged this value into the initial equation: and got that 0.00000134 moles of Nitrogen.
Nitrogen's molar mass is 14.0674 which means that:
.00001877 grams of nitrogen are required.
So, this is the long way. I didn't think to look up the density of Nitrogen at 1bar and see how much 32865 cubic millimeters of it would be.
the density of nitrogen at 101321Pa is 1.251g/L
which is .000001251 g/mm^3
multiply that by 32865 mm^3
So, .04 grams of nitrogen!
What else can I help you with?
What is the pressure inside of a container when nitrogen gas is added?
The pressure inside of a container when nitrogen gas is added depends on:what the pressure was before the gas was addedhow big the container ishow much nitrogen gas is addedthe temperature of the gas before it is addedthe temperature of the container and its contents
Is nitrogen gas soluble in water when pressure is halved?
Solubilty of gases in water increase when the temperature decrease, For nitrogen you can see an infographics at this link.
If nitrogen were pumped into your lungs at high pressure what would happen to its solubility in your blood?
If nitrogen were pumped into your lungs at high pressure, its solubility in your blood would increase due to Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. This could lead to nitrogen bubbles forming in the bloodstream, causing decompression sickness or "the bends."
Why pressure decrease with increase in humidity?
An increase in humidity causes the air to become less dense, which results in a decrease in pressure. This is because water vapor molecules displace nitrogen and oxygen molecules in the air, reducing the overall mass of air and lowering the pressure.
Is nitrogen gas at high temperature and pressure flammable is there is no temperature and pressure at which nitrogen gas can be flammable?
Nitrogen gas is not in itself flammable, and does not have an auto ignition temperature.
When charging a system with a low pressure control and the control keeps shutting the compressor off you should?
When charging a system with a low pressure control and the control keeps shutting the compressor off, you should:
What will be the result if you increase the pressure on one liter of nitrogen?
Increasing the pressure on one liter of nitrogen will cause the volume to decrease while the temperature remains constant, according to Boyle's Law. The relationship between pressure and volume is inversely proportional, meaning that as pressure increases, volume decreases.
What is the pressure inside of a container when nitrogen gas is added?
The pressure inside of a container when nitrogen gas is added depends on:what the pressure was before the gas was addedhow big the container ishow much nitrogen gas is addedthe temperature of the gas before it is addedthe temperature of the container and its contents
What happen when you increase the pressure of nitrogen beyond the critical pressure and will it still exist in liquid phase?
The state of an element is a function of both pressure and temperature.
Is nitrogen gas soluble in water when pressure is halved?
Solubilty of gases in water increase when the temperature decrease, For nitrogen you can see an infographics at this link.
If nitrogen were pumped into your lungs at high pressure what would happen to its solubility in your blood?
If nitrogen were pumped into your lungs at high pressure, its solubility in your blood would increase due to Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. This could lead to nitrogen bubbles forming in the bloodstream, causing decompression sickness or "the bends."
Why pressure decrease with increase in humidity?
An increase in humidity causes the air to become less dense, which results in a decrease in pressure. This is because water vapor molecules displace nitrogen and oxygen molecules in the air, reducing the overall mass of air and lowering the pressure.
Can liquid nitrogen evaporate from a sealed container?
Yes, liquid nitrogen can evaporate from a sealed container due to its low boiling point of -196°C. The pressure will increase in the container as the liquid nitrogen evaporates, eventually leading to a rupture or explosion if the container is not designed to handle the buildup of pressure.
A sample of nitrogen gas is collected over water at 20 degrees Celsius. The vapor pressure of water at 20 degrees Celsius is 18 mmHg. What is the partial pressure of the nitrogen if the total pressure?
The total pressure is the sum of the partial pressure of nitrogen and the vapor pressure of water. Therefore, the partial pressure of nitrogen is the total pressure minus the vapor pressure of water. Given that the total pressure is not provided in the question, we need more information to calculate the partial pressure of nitrogen.
A barometer shows the atmospheric pressure to be 762 mm Hg What is the partial pressure of nitrogen if nitrogen is 78 percent of the air?
To find the partial pressure of nitrogen, multiply the atmospheric pressure by the percentage of nitrogen in the air (0.78). Therefore, the partial pressure of nitrogen would be 0.78 * 762 mm Hg, which equals 594.36 mm Hg.
Is nitrogen a compressed gas?
Nitrogen can exist as a compressed gas when placed under pressure in a container. At room temperature and normal atmospheric pressure, nitrogen is a colorless and odorless gas.
What is the relationship between temperature and pressure that affects the nitrogen gas density?
The relationship between temperature and pressure that affects the density of nitrogen gas is described by the ideal gas law. According to this law, as temperature increases, the pressure of the gas also increases, leading to a decrease in gas density. Conversely, as temperature decreases, the pressure decreases, resulting in an increase in gas density.
