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To compress nitrogen at 1 ATM from 750 mL to 500 mL what must the new pressure be if the temperature is kept constant?
To find the new pressure when compressing nitrogen at constant temperature, you can use Boyle's Law, which states that ( P_1V_1 = P_2V_2 ). Given ( P_1 = 1 ) ATM, ( V_1 = 750 ) mL, and ( V_2 = 500 ) mL, you can rearrange the equation to solve for ( P_2 ): ( P_2 = \frac{P_1V_1}{V_2} = \frac{1 , \text{ATM} \times 750 , \text{mL}}{500 , \text{mL}} = 1.5 ) ATM. Thus, the new pressure must be 1.5 ATM.
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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.
What pressure must be used to compress 850 mL of argon gas at 146 kPa to 150 mL Temperature is held constant?
The initial and final volumes of the gas are related by Boyle's Law: (P_1V_1 = P_2V_2). Therefore, the pressure needed to compress 850 mL of argon gas at 146 kPa to 150 mL, with temperature constant, is calculated as follows: (P_2 = \frac{P_1V_1}{V_2} = \frac{146 \text{ kPa} \times 850 \text{ mL}}{150 \text{ mL}} = 825.33) kPa. Thus, a pressure of approximately 825.33 kPa is required for compression.
What happens to the gas volume at a given pressure?
The gas takes on the size and shape of the container it's in. So if you make the volume of the container smaller (compress it) the volume of the gas is smaller as well. However, this comes at a higher pressure exerted, so there is no spontaneous mass creation.Well, by definition, compress means "to make smaller; to press or squeeze together; or to make something occupy a smaller space or volume." Therefore, the very word "compress" implies a decrease in volume. So if you wanted to know what happens when you compress a gas, you are squeezing it into a smaller space, or decreasing the volume.If you were to let the gas maintain a constant temperature as you compress it, then pressure would increase. If you were to let the gas maintain a constant pressure, then temperature would decrease.If you were to rephrase your question to "what happens to the volume of gas if put under pressure," then the gas' volume would decrease. For the temperature to remain constant and the pressure to increase, a gas must decrease in volume to occupy a smaller area.
What must the temperature be for the gas to remain at a constant pressure?
"Constant pressure" means the pressure must not change.
What happens to a gas temperature at a given pressure?
In a closed system with constant pressure and no input or output of heat, the gas temperature will remain constant. In that same system, if the pressure is increased, then the gas temperature will also increase. If pressure is decreased, then the gas temperature will decrease.
What happens to volume when temperature of gas is decresd at constant pressure?
If the temperature of the gas is decreasing, then in order to maintain constant pressure, you would have to compress it in volume.
Does Nitrogen PSI change with temperature?
Yes, the pressure of nitrogen gas will change with temperature according to the ideal gas law. As temperature increases, the pressure of nitrogen gas will also increase, assuming the volume and amount of gas remain constant. Conversely, a decrease in temperature will result in a decrease in pressure, as long as other factors remain constant.
Is oxygen free nitrogen pressure affected by temperature?
Yes, the pressure of oxygen-free nitrogen is affected by temperature. As temperature increases, the pressure of a gas also increases if the volume and amount of gas are constant, according to the ideal gas law. Conversely, as temperature decreases, the pressure decreases.
If the temperature remains constant800 mL of nitrogen at 2.0 ATM must be compressed to what pressure to reach 500 ml?
To calculate the new pressure required to compress the nitrogen to 500 mL from 800 mL at a constant temperature, we can use Boyle's Law, which states that pressure and volume are inversely proportional. We can set up the equation as (800 mL) * (2.0 ATM) = (500 mL) * (P), where P is the new pressure. Solving for P, the new pressure required would be 3.2 ATM.
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.
How do you ake liquid nitrogen?
The first principle: Nitrogen liquifies at -196C, and air contains a lot of nitrogen. So you're going to get your liquid nitrogen out of air, right?The second principle: If you compress air it heats up, and if you release the pressure it loses that heat--principle of entropy at work. Good so far?The third principle is how this really works: if you compress the air, cool it down while it's compressed, and then release the pressure it will get even colder. So what you do is very simple: compress air, cool it and release the pressure. As the temperature of the air drops during pressure release, eventually it will pass through the magic -196C point and the nitrogen will condense out of it.
When the pressure of a gas increases at constant temperature its volume?
Temperature increases as pressure increases.
When the temperature of of gas increases at constant pressure its?
As pressure increases, if temperature is constant, the gas will decrease in volume.
What pressure must be used to compress 850 mL of argon gas at 146 kPa to 150 mL Temperature is held constant?
The initial and final volumes of the gas are related by Boyle's Law: (P_1V_1 = P_2V_2). Therefore, the pressure needed to compress 850 mL of argon gas at 146 kPa to 150 mL, with temperature constant, is calculated as follows: (P_2 = \frac{P_1V_1}{V_2} = \frac{146 \text{ kPa} \times 850 \text{ mL}}{150 \text{ mL}} = 825.33) kPa. Thus, a pressure of approximately 825.33 kPa is required for compression.
When the temperature is constant will the the volume of a gas decrease as the pressure decreases?
At constant temperature p.V=constant, so pressure INcreases when decreasing the volume.
What happens to the gas volume at a given pressure?
The gas takes on the size and shape of the container it's in. So if you make the volume of the container smaller (compress it) the volume of the gas is smaller as well. However, this comes at a higher pressure exerted, so there is no spontaneous mass creation.Well, by definition, compress means "to make smaller; to press or squeeze together; or to make something occupy a smaller space or volume." Therefore, the very word "compress" implies a decrease in volume. So if you wanted to know what happens when you compress a gas, you are squeezing it into a smaller space, or decreasing the volume.If you were to let the gas maintain a constant temperature as you compress it, then pressure would increase. If you were to let the gas maintain a constant pressure, then temperature would decrease.If you were to rephrase your question to "what happens to the volume of gas if put under pressure," then the gas' volume would decrease. For the temperature to remain constant and the pressure to increase, a gas must decrease in volume to occupy a smaller area.
When the temperature of a gas increases at constant pressure it's?
As pressure increases, if temperature is constant, the gas will decrease in volume.
