1875 mL
Using Boyle's Law (P1V1 = P2V2), you can calculate the new volume at the room pressure of one atmosphere. V2 = (P1V1)/P2 = (7.50 atm * 250 ml) / 1 atm = 1875 ml.
To calculate the volume of the cylinder at 1 atmosphere, you would need to convert the pressure to atmospheres (1 atm is approximately 101325 Pa), then apply the ideal gas law (PV = nRT) to find the new volume with the new pressure. Given that pressure is 150 N/m^2 and the original volume is 6 cubic meters, further calculations are needed for an accurate answer.
If the volume of the container is reduced to 1.80 L, the pressure inside the container will increase according to Boyle's Law, which states that pressure and volume are inversely proportional when temperature is constant. The pressure will increase because the volume is decreasing.
The volume of gas at a depth of 100 feet would depend on the pressure and temperature at that depth. As pressure increases with depth, gas volume decreases. To calculate the exact volume, you would need to know the specific pressure and temperature conditions at that depth.
When a gas expands and its volume increases, the pressure of the gas will decrease. This is because pressure and volume are inversely proportional according to Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume at constant temperature.
Argon makes up about 0.93% of the Earth's atmosphere by volume.
Atmospheres cannot be converter to milliliters. Atmospheres are a unit of pressure based on the Earth's atmosphere. Milliliters are a unit of volume, otherwise known as a cubic centimeter.
You don't. Liters is a unit of volume, atmospheres is a unit of pressure.
To calculate the volume of the cylinder at 1 atmosphere, you would need to convert the pressure to atmospheres (1 atm is approximately 101325 Pa), then apply the ideal gas law (PV = nRT) to find the new volume with the new pressure. Given that pressure is 150 N/m^2 and the original volume is 6 cubic meters, further calculations are needed for an accurate answer.
The pressure is 172,84 atmospheres.
If the volume of the container is reduced to 1.80 L, the pressure inside the container will increase according to Boyle's Law, which states that pressure and volume are inversely proportional when temperature is constant. The pressure will increase because the volume is decreasing.
For this you would use Boyle's Law, P1V1 = P2V2. The first pressure and volume variables are before the change, while the second set are after the change. In this case, the volume is being changed and the pressure has to be solved for. P1 = 1.00 ATM V1 = 2.0 L P2 = Unknown V2 = 4.00 L P1V1 = P2V2 1.00(2.0)=4.00P P= .5 ATM
The equation is P1V1=P2V2. (P1 is pressure before the change, P2 is the pressure after, V1 is the volume before the change, and V2 is the volume after it.) So to solve it, it would be the same change no matter how much the volume and pressure were to begin with. The values are P1= 1 atmosphere (the pressure of air at sea level) V1= 1 Liter which would mean P2=3 atmospheres 1*1=3(V2) 1/3 Liter= V2. So the volume would be one third of what it was before the pressure was tripled.
atmospheres
The volume of gas at a depth of 100 feet would depend on the pressure and temperature at that depth. As pressure increases with depth, gas volume decreases. To calculate the exact volume, you would need to know the specific pressure and temperature conditions at that depth.
At standard temperature and pressure (STP) of 0°C and 1 atmosphere, 1 mole of any ideal gas occupies 22.4 liters of volume. This applies to nitrogen gas as well.
75 atmospheres of pressure is 1125 pounds per square inch. A balloon would be unlikely to withstand this pressure.
The answer is 13,89 moles.