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What is the volume 0.323-mol sample of gas will occupy at 265k and pressure of 0.900atm?
To solve this problem, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. Rearranging the equation to solve for V, we get V = (nRT)/P. Plugging in the values given (n = 0.323 mol, T = 265 K, P = 0.900 atm, and R = 0.0821 L.atm/mol.K), we can calculate the volume of the gas.
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A sample of oxygen gas occupies 320.0 mL at 27C and atmospheric pressure What volume does it occupy at 120C and the same pressure?
419 mL
Under what sets of conditions will a 0.50 mole sample of helium occupy a volume of 11.2 liters?
At STP, 1 mole of a gas will occupy 22.4 liters; or 0.5 mole will occupy 11.2 liters.
Under what sets of condition will a 0.50 mole sample of helium occupy a volume of 11.2 liters?
A 0.50 mole sample of helium will occupy a volume of 11.2 liters under standard temperature and pressure (STP) conditions, which are 0 degrees Celsius (273.15 K) and 1 atmosphere pressure. At STP, one mole of any gas occupies a volume of 22.4 liters.
What is the volume 0.323 mol sample of gas will occupy at 265k and pressure of 0.900atm?
Using the ideal gas law, V = (nRT)/P, where V is volume, n is moles, R is the gas constant, T is temperature in Kelvin, and P is pressure, we can calculate the volume to be 7.34 L.
Why you use chilled sample in Reid vapor pressure method?
Chilling the sample in the Reid vapor pressure test helps to reduce the vapor pressure of the volatile components in the sample, making it easier to measure accurately. This allows for more precise determination of the vapor pressure under controlled conditions.
A sample of oxygen gas occupies 300.0 mL at 27ºC and atmospheric pressure What volume does it occupy at 150ºC and the same pressure?
423mL
A sample of oxygen gas occupies 320.0 mL at 27C and atmospheric pressure What volume does it occupy at 120C and the same pressure?
419 mL
Under what sets of conditions will a 0.50 mole sample of helium occupy a volume of 11.2 liters?
At STP, 1 mole of a gas will occupy 22.4 liters; or 0.5 mole will occupy 11.2 liters.
Under what sets of condition will a 0.50 mole sample of helium occupy a volume of 11.2 liters?
A 0.50 mole sample of helium will occupy a volume of 11.2 liters under standard temperature and pressure (STP) conditions, which are 0 degrees Celsius (273.15 K) and 1 atmosphere pressure. At STP, one mole of any gas occupies a volume of 22.4 liters.
What will happen if the pressure on a sample of gas is raised three times and it's temperature is kept constant?
If the pressure on a sample of gas is raised three times and the temperature is kept constant, according to Boyle's Law, the volume of the gas will decrease proportionally to maintain a constant temperature. This means the gas will be compressed and occupy a smaller volume.
A gas sample occupies 4.2 L at a pressure of 101 kPa. What volume will it occupy if the pressure is increased to 235 kPa?
More pressure means less volume. Calculate the ratio of pressure, then divide the 4.2 liters by that ratio.This assumes: * That the temperature doesn't change. * That the gas behaves like an ideal gas.
What is the volume 0.323 mol sample of gas will occupy at 265k and pressure of 0.900atm?
Using the ideal gas law, V = (nRT)/P, where V is volume, n is moles, R is the gas constant, T is temperature in Kelvin, and P is pressure, we can calculate the volume to be 7.34 L.
If a sample of gas occupies 20 ml at -132 C what volume does the sample occupy at 50 C?
To find the new volume, you can use the combined gas law formula: (P1 * V1) / T1 = (P2 * V2) / T2. Since pressure is constant, it can be eliminated. Rearrange the formula to solve for V2: V2 = (V1 * T2) / T1. Plug in the values: V2 = (20 ml * 323 K) / 141 K = 45.1 ml. So, the sample of gas would occupy 45.1 ml at 50 C.
Why you use chilled sample in Reid vapor pressure method?
Chilling the sample in the Reid vapor pressure test helps to reduce the vapor pressure of the volatile components in the sample, making it easier to measure accurately. This allows for more precise determination of the vapor pressure under controlled conditions.
What happens to the partial pressure of oxygen in a sample of air when the temperature increases?
When the temperature of a sample of air increases, the partial pressure of oxygen also increases.
Which sample of water has the lowest vapor pressure?
The sample of water that has the lowest vapor pressure is the sample at a lower temperature. Vapor pressure decreases as temperature decreases because fewer molecules have enough energy to escape into the gas phase.
What volume would a 0.871 gram sample of air occupy if the density of air is 1.29g ml?
multiply the mass and the density
