A 0.49 mol sample of oxygen is in a 4.8 L container at 25 ºC. What is the pressure in the container?
a)254 atm
b)8.6 atm
c)2.5 atm
d)0.40 atm
A 0.49 mol sample of oxygen is in a 4.8 L container at 25 ºC. What...
A 10.74 mol sample of oxygen gas is maintained in a 0.8354 L container at 296.1 K. What is the pressure in atm calculated using the van der Waals' equation for O2 gas under these conditions? For 02, a = 1.360 Latm/mo12 and b = 3.183x10-2 L/mol. atm
Acetone, C3H6O, has a vapor pressure of 0.307 bar at 25 ºC. A sample of 0.100 mol acetone is added to a container that contains 1.00 L of argon gas at 1.00 bar pressure and 25 ºC. The volume of the container is then increased to 4.00 L while maintaining the same temperature. What is the pressure in the container after the expansion? It is supposed to be C but I am not sure why. (A) 0.250 bar (B) 0.307...
Question 21 a)b)c) A(n) 8.87-mol sample of carbon monoxide was stored in a 30.0-L container at 48.5°C. What is the pressure of the carbon monoxide in the container? Enter your answer in the box provided. atm The temperature of a gas is initially 67.0°C. What temperature is needed to double the volume of the gas if mass and pressure do not change? Enter your answer in the provided box. A 30.0-L gas cylinder contains 4.90 g H, at 25°C. What...
A 10.33 mol sample of krypton gas is maintained in a 0.7797 L container at 301.0 K. What is the pressure in atm calculated using the van der Waals' equation for Kr gas under these conditions? For Kr, a = 2.318 L’atm/mol and b = 3.978x10-2 L/mol. atm
A 0.49 g sample of an ideal gas in a 200 ml container at 26 °C exerts a pressure of 0.98 atm. What is the molar mass of this gas (in g/mol)? NOTE: The molar mass you calculate may not correspond to a real-life gas (don't try to identify the gas). You have 5 attempts at this question. Answer: Check
1. What is the partial pressure of nitrogen in a container that contains 5.82 mol of oxygen, 7.90 mol of nitrogen, and 5.85 mol of carbon dioxide when the total pressure is 621 mmHg? A) 185 mmHg B) 186 mmHg C) 251 mmHg D) 420 mmHg E) 621 mmHg 2. Using the van der Waals equation, determine the pressure of 335.0 g of SO2(g) in a 5.70-L vessel at 661 K. For SO2(g), a = 6.865 L2 • atm/mol2 and...
According to the ideal gas law, a 0.9100 mol sample of oxygen gas in a 1.139 L container at 272.3 K should exert a pressure of 17.85 atm. What is the percent difference between the pressure calculated using the var der Waals' equation and the ideal pressure? For O2 gas, a=1.360 L2 atm/mol2 and b=3.183x10-2 L mol. Using Percent Difference Formula?
A 9.450 mol sample of krypton gas is maintained in a 0.8100 L container at 300.1 K. What is the pressure in atm calculated using the van der Waals' equation for Kr gas under these conditions? For Kr, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. atm
If a sample of oxygen gas, originally at 5.00 atm in 1.00 L, is heated in that container from 25.0°C to 175°C, what is the final pressure? A: 7.52 atm B: 0.714 atm C: 0.133 atm D: 35.0 atm
Consider 0.05 mol of diatomic Oxygen in a container with initial volume 1 L and initial pressure 1 atm. The Oxygen undergoes an adiabatic compression until its final pressure is 3 atm. Assume that the two rotational degrees of freedom are active, but the vibrational degrees are frozen out i) What is the final volume of the gas? ii) Calculate the work done on the gas and the heat added during this process. iii) What is the change in the...