Suppose you have 0.664 mol of an ideal gas in a 0.454 L container at 39.97 atm. a) What is the temperature of this gas? b) Sketch a pressure versus volume graph for this ideal gas, either using the graph paper on the next page or in a spreadsheet such as Excel. Have the graph go out to 4 L and 70 atm. Use at least 6 points to draw this curve. c) On the graph from part b, use a dotted line to sketch the approximate curve that you might expect to see for a real gas with strong repulsive intermolecular interactions at high pressures (i.e. above 10 atm).
Suppose you have 0.664 mol of an ideal gas in a 0.454 L container at 39.97...
Suppose 10.00 mol of Ar gas are pumped into a 1.01 L container at 293.15 K. Calculate the expected pressure based on the ideal gas law, Pideal. ?atm Calculate an estimate of the gas pressure one might observe based on the van der Waals equation, Pobs. a = 1.34 L2 · atm/mol2, b = 0.0322 L/mol. atm Part 3 (1 point) Which factor, a or b, is the primary reason for the difference in the calculated pressures? Choose one: a....
Imagine that you have an ideal gas in a 4.70 L container, and that 2750 molecules of this gas collide with a square-inch area of the container at any given instant. If the volume is increased to 18.8 L at constant temperature, how many collisions will occur per square inch of this larger container?
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
Imagine that you have an ideal gas in a 6.90 L container, and that 1350 molecules of this gas collide with a square-inch area of the container at any given instant. If the volume is increased to 55.2 L at constant temperature, how many collisions will occur per square inch of this larger container? Enter the number of collisions per square inch.
Hint: % difference = 100×(P ideal - Pvan der Waals) / P idealAccording to the ideal gas law, a 9.843 mol sample of argon gas in a 0.8425 L container at 502.0 K should exert a pressure of 481.3 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Ar gas, a =1.345L2 atm/mol2 and b = 3.219×10-2 L/mol.
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...
A sealed container holding 0.0255 L of an ideal gas at 0.987 atm and 69 °C is placed into a refrigerator and cooled to 43 °C with no change in volume. Calculate the final pressure of the gas. P= atm I help contact us careers about us | privacy policy terms of use e D TI
You have a 3.00-L container filled with N₂ (MM = 28.02 g/mol) at 298.15 K and 1.75 atm pressure connected to a 2.00-L container filled with Ar (MM = 39.95 g/mol) at 298.15 K and 2.15 atm pressure. A stopcock connecting the containers is opened and the gases are allowed to equilibrate between the two containers. What is the density of the final gas mixture? Assume ideal behavior. (Use R = 0.08206 L.atm/mol.K) (HINT: What is the total mass, m,...
Suppose you have a fixed container containing 0.255 moles of a gas (the identity of the gas doesn't matter). If the container volume is 0.748 L, and the temperature is 301.15 K, what is the pressure in atm? (R=0.0821 L'atm/mol-K) O A.0.784 atm OB. 0.00842 atm O C.7.84 x 104 atm D.8.42 atm
The volume of 3.3 mol of ideal gas is 45.7 L at 350 K. Calculate its pressure (in atmospheres). L atm L kPa • Use R = 0.08206 314 for the ideal gas constant. mol K Your answer should have two significant figures. Do NOT include units in your response. mol K for the Provide your answer below: