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What is the volume occupied by 20.4 liters of co2 at 1200 torr when it is STP?
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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
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 are the most common units of pressure volume and temperature?
pressure -- Torr which is equivalent to mmHg, Pascals or kPa, atmospheres, psi, inches Hg Volume -- usually liters Temperature -- Kelvin or Celsius which must be converted to Kelvin to be used in any gas law equations
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 37.7 ml volume of an unknown gas is collected over water at 19 degrees celsius and a total pressure of 770 torr The mass of the gas is 68.6 mg What volume does the gas occupy?
the gas occupies a volume of37.7 ml as stated in the question either your question is wrong or incomplete.
What volume is occupied by 1.00 kg of helium at 5.00 degrees celsius at a pressure of 735 torr?
Well, we might as well convert all of this mess. ( we could work in Torr, but why when we are mass converting )1.00 kg He (1000 grams/1 kg) = 1000 grams He (1 mole He/4.003 grams) = 250 moles He5.00o Celsius = 278.15 Kelvin735 Torr = (1 atm/760 Torr = 0.967 atmospheres=========================================Now,PV = nRT(0.967 atm)(Volume) = (250 moles He)(0.08206 L*atm/mol*K)(278.15 K)0.967V = 5706.247Volume = 5.90 X 103 Liters-----------------------------------
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
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
Which equation is set up correctly to determine the volume of a 1.5 mole sample of oxygen gas at 22C and 100 kPa?
The ideal gas equation.PV = nRT22o C = 295.15 Kelvin(750 Torr)(X volume) = (1.5 moles O2)(62.36 L*torr/mol*K)(295.15 K)Volume = 27608.331/750= 37 Liters oxygen gas=================
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
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 are the most common units of pressure volume and temperature?
pressure -- Torr which is equivalent to mmHg, Pascals or kPa, atmospheres, psi, inches Hg Volume -- usually liters Temperature -- Kelvin or Celsius which must be converted to Kelvin to be used in any gas law equations
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.
What is the new pressure of 150 ml of a gas that is compressed to 50 ml when the original pressure was 3.0atm?
You have to convert the temperature to Kelvins, the volume to liters, and the pressure to torr. You use the combined gas law and solve for pressure. P1V1/T1 = P2V2/T2 P1 = P2V2T1/T2V1 P1 = (608 torr)(0.300 L)(323.15 K) / (310.15 K) (0.555 L) P1 = 342.42 torr I believe that if you are using the correct number of significant digits, you would write the answer as 342 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.
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.
