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A sample of propane a component of LP gas has a volume of 35.3 L at 315 K and 922 torr What is its volume at STP?
Wiki User
∙ 13y ago
37.1L is the answer
Wiki User
∙ 13y ago
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What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2 degrees C when it occupies a volume of 5.00 L?
The pressure is 39,8 torr.
A 200 ml sample of hydrogen is collected over water at 745.5 torr and 290K If the vapor pressure of water at 290k is 14.5 torr What is the volume of dry hydrogen at STP The answer is 181m?
I believe u mean mL, m is not a unit of volume
A 325-mL sample of air is at 810.5 torr and 30.0 C What volume mL will this gas occupy at 900.0 torr and 60.0 C?
I got 321.6mL. You use PV=nRT to find n, and plug that into PV=nRT with the new conditions to find the new volume.
When a sample of neon with a volume of 648 mL and a pressure of 0.985 ATM was heated from 16.0 to 63.0 C its volume became 689 mL What was its final pressure in ATM?
Begin with the Equation; P1V1/ T1 = P2V2/ T2 Therefore, (785 torr)(2.00 L) / (37.0 C) = (X)(3.24 L)/ (58.0 C) = 759.59 TORR. To get the answer into ATM, you need to divide the answer in torr by 760. EX. 760torr = 1 atm. 759.59 torr / 760 torr = .999 atm.
As the pressure of a gas at 760 torr is changed to 380 torr at a constant temperature the volum of the gas will?
Boyle's law states that pressure is indirectly proportional to the volume. There fore as the pressure of a gas at 760 torr is changed to 380 torr, the volume will increase. Boyle's Law: P1 x V1 = P2 x V2 Rearranging leads to: P1 / P2 = V2 / V1 Substituting our values: 760 / 380 = V2 / V1 Thus the final volume will be twice the initial volume.
A 125.0 mL sample of nitrogen at 790 torr was compressed to a volume of 75.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
1300<--- torr
A 110.0 mL sample of nitrogen at 820 torr was compressed to a volume of 83.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
1100
A 100.0 mL sample of nitrogen at 810 torr was compressed to a volume of 72.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
1100
What will be the final volume of a 500 ml sample of helium if its pressure is changed from 740 Torr to 780 Torr and its temperature is kept constant?
P1V1 = P2V2 (740 torr)(500 ml) = (780 torr)V2 V2 = (740 torr)(500 ml) / (780 torr) V2 ~ 474 ml
What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2 degrees C when it occupies a volume of 5.00 L?
The pressure is 39,8 torr.
A 100 ml sample of nitrogen at 810 torr was compressed to a volume of 72 mL in a syringe What was the pressure of trapped nitrogen in torr?
P1*V1 = P2*V2, Therefore your numerical answer would be 100*810/72 torr.
A 200 ml sample of hydrogen is collected over water at 745.5 torr and 290K If the vapor pressure of water at 290k is 14.5 torr What is the volume of dry hydrogen at STP The answer is 181m?
I believe u mean mL, m is not a unit of volume
A 325-mL sample of air is at 810.5 torr and 30.0 C What volume mL will this gas occupy at 900.0 torr and 60.0 C?
I got 321.6mL. You use PV=nRT to find n, and plug that into PV=nRT with the new conditions to find the new volume.
When a sample of neon with a volume of 648 mL and a pressure of 0.985 ATM was heated from 16.0 to 63.0 C its volume became 689 mL What was its final pressure in ATM?
Begin with the Equation; P1V1/ T1 = P2V2/ T2 Therefore, (785 torr)(2.00 L) / (37.0 C) = (X)(3.24 L)/ (58.0 C) = 759.59 TORR. To get the answer into ATM, you need to divide the answer in torr by 760. EX. 760torr = 1 atm. 759.59 torr / 760 torr = .999 atm.
a gas has a pressure of 766.7 torr at a temperature of 10.0°C. the sample contains 2.35 moles of xenon. what is the volume of the gas in liters?
Using PV=nRT, 10.0ºC = 283.15ºK, R = 62.36 L torr/mol K V= (nRT)/P V = (2.35m*(62.36 L torr/mol K)*283.15ºK)/766.7 Torr V = 54.12 L
As the pressure of a gas at 760 torr is changed to 380 torr at a constant temperature the volum of the gas will?
Boyle's law states that pressure is indirectly proportional to the volume. There fore as the pressure of a gas at 760 torr is changed to 380 torr, the volume will increase. Boyle's Law: P1 x V1 = P2 x V2 Rearranging leads to: P1 / P2 = V2 / V1 Substituting our values: 760 / 380 = V2 / V1 Thus the final volume will be twice the initial volume.
A closed end manometer has a U tube with a sample of hydrogen gas in the bulb The difference in the height of the columns of mercury is 18.0 cm What is the pressure of the hydrogen gas in torr?
140 torr
