At 273 K, 1.00 mol of an ideal gas confined to a 2.00-L container exerts a pressure of 11.2 atm. Under the same conditions, what pressure is exerted by CO2, for which a = 3.59 L2 atm mol-2 and b = 0.0427 L mol-1 0 -0.90 10.5 09.1 O 7.2 11.4
If 34.5 mol of an ideal gas is at 5.25 atm and 393 K, what is the volume of the gas? volume: L
If 75.5 mol of an ideal gas is at 3.55 atm and 403 K, what is the volume of the gas? volume: L
If 70.5 mol of an ideal gas is at 3.47 atm at 52.50 C, what is the volume of the gas? L V = A sample of an ideal gas has a volume of 2.30 L at 283 K and 1.10 atm. Calculate the pressure when the volume is 1.08 L and the temperature is 305 K P = atm
1.Ideal Gas Law PV = nRT with atm: R = 0.0821 L*atm/(K*mol) If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 2. If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container? 3. If I have 7.7 moles of gas at a pressure of 0.09...
If 75.5 mol of an ideal gas is at 3.55 atm and 403 K, what is the volume of the gas? volume:
If 35.5 mol of an ideal gas is at 2.47 atm and 465 K, what is the volume of the gas?
If 80.5 mol of an ideal gas is at 5.79 atm and 387 K, what is the volume of the gas?
If an ideal gas has a pressure of 3.83 atm, a temperature of 445 K, and a volume of 24.75 L, how many moles of gas are in the sample? mol
Question 1 (a) Use the ideal gas equation to calculate the pressure (in atm) of 2.40 mol of krypton (Kr) at 455 K in a 4.50 L vessel. (b) In a 16.3 L vessel, the pressure of 2.40 mol of Kr at 455 K is 5.50 atm when calculated using the ideal gas equation and 5.40 atm when calculated using the van der waals equation of state (Note: a=5.121 and b = 0.0106). Why is the percent difference in the...