A sample of neon gas at 795 torr and 60.0 L is compressed to 48.5 L....
A sample of gas at 760 torr and 2.8 L is compressed at constant temperature to the pressure at 3.5 atm. What is the final volume of the gas? My biggest problem with answering this question is the fact that I don't know what the "constant temperature" is..I know I'm using the combined gas law with formula: V2= p1v1/t1p2 * T2 and that p1=760 torr or 1 atm, v1=2.8L and p2=3.5 atm... Any help on this is very much appreciated.
A sample of gas initially occupies 3.50 L at a pressure of 795 torr at 32°C. What will the temperature be if the pressure is changed to 4.00 atm, and the volume is changed to 1.50 L?
At 20°C, a sample of gas has a volume of 2.51 L at 795 torr. What is the new pressure (in atm) if the volume is increased to 6.46 L at the same temperature?
A sample of neon gas at a pressure of 820 torr and a temperature of 24.5 °C, occupies a volume of 848 mL. If the gas is allowed to expand at constant temperature until its pressure is 524 torr, the volume of the gas sample will be ---- mL.
A 99.3 g sample of O2 gas at 0.0 oC and 380 Torr is compressed and heated until the volume is 3.99 L and the temperature is 27 oC. What is the final pressure in Torr? The number of significant digits is set to 3
A sample of Ar gas with a volume of 48.6 mL at 610 torr is compressed at constant temperature until its volume is 32.7 mL. What will be the new pressure of the sample in torr?
1) a sample of nitrogen gas at a pressure of 795 mm Hg and a temp of 84•C occupies 69.79 liters. If the gas is cooled at constant pressure to a temp of 39•C the volume of the gas sample will be __ L 2)A sample of neon gas at a pressure of 0.905 atm and a temperature of 238 °C, occupies a volume of 461 mL. If the gas is heated at constant pressure until its volune is 572...
Using the same sample of gas ( P 1 = 795 torr , T 1 = 25 ∘ C ), we wish to change the pressure to 7950 torr with no accompanying change in volume or amount of gas. What temperature T 2 , in Celsius, is needed to reach this pressure?
A sample of oxygen gas occupies 1.9 L at pressure of 1156 torr. What volume will it occupy when the pressure is changed to 912 torr and temperature remains constant?
A sample containing 3.00 moles of neon gas has a volume of 7.00 L . Assume that the pressure and the temperature remain constant. (Help Please ASAP!) i. What is the new volume of gas in liters when a leak allows one-half of the neon atoms to escape? ii. What is the new volume of gas in liters when a sample of 60.0 g of neon is added to the 3.00 moles of neon gas already in the container? iii....