At 273 K, 1.00 mol of an ideal gas confined to a 2.00-L container exerts a...
Be sure to answer all parts. Calculate the pressure exerted by 2.65 moles of CO2 confined in a volume of 4.03 L at 456 K. What pressure is predicted by the ideal gas equation? The van der Waals constants for CQ area 3.59 atm. L2/mol2 and b 0.0427 L/mol. van der Waals equation: ideal gas equation: [24.6 ]atm
3.45 mol of CO2(g) is confined to a volume of 5.00L at 450.K. This results in high pressure and non-ideal gas behavior. Determine the pressure in units of atm. Per Table 5.4 in the textbook, a = 3.59 atm·L2/mol2 and b = 0.0427 L/mol.
A gas is confined in a container with flexible walls, like a balloon. At 273 K and 5 atm of pressure, the volume of the gas is 10.0 L. If the pressure remains constant while the temperature decreases to 250 K, you would expect the volume of the gas to _____. Increase Vary Widely Remain Constanst Decrease
The ideal pressure of 1.00 mol CH3Cl gas in a 4.50 L flask at 100.0 K is 1.82 atm. What is its real pressure? For CH3Cl: a = 7.570 atm∙L2 /mol2 b = 0.06483 L/mol a. 1.27 atm b. 1.45 atm c. 1.48 atm d. 1.51 atm e. 1.58 atm
2. (15pts) Calculate the pressure exerted by 1.0 mol C2Ho behaving as i) as an ideal gas ii) as a van der Waals gas when it is confined under the following conditions: at 600 K in 200 cm3. (For C2Ho:a-5.507 atm dm mor2 and b-6.51x102 dm3 mor') 2. (15pts) Calculate the pressure exerted by 1.0 mol C2Ho behaving as i) as an ideal gas ii) as a van der Waals gas when it is confined under the following conditions: at...
If 1.00 mol of argon is placed in a 0.500-L container at 30.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol.
3) The temperature of an ideal gas confined in a 5 L container is raised from 20 °C to 70 °C. If the initial pressure of the gas was 1.5 atm, what is the final pressure of the gas?
If 1.00 mol of argon is placed in a 0.500-L container at 30.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol. Express your answer to two significant figures and include the appropriate units.
If 1.00 mol of argon is placed in a 0.500-L container at 22.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol. Express your answer to two significant figures and include the appropriate units.
A sample of 18 g of oxygen gas (O2) is confined in a container at 200 kPa and 273 K. The gas is allowed to expand adiabatically and reversibly to 100 kPa. Calculate the final temperature of the gas. The molar heat capacity at constant pressure (CP,m) of O2 is 29.355 J mol-1 K-1