If 2.00 mol of nitrogen gas (N2) are placed in a cubic box, 24.0 cm on each side, at 1.50 atm of pressure, what is the rms speed of the nitrogen molecules?
If 2.00 mol of nitrogen gas (N2) are placed in a cubic box, 24.0 cm on...
If 2.00 mol of nitrogen gas (N2) are placed in a cubic box, 24.0 cm on each side, at 1.50 atm of pressure, what is the rms speed of the nitrogen molecules?
A cubic container of volume 2.00 L holds 0.500 mol of nitrogen gas at a temperature of 25.0°C. What is the net force due to the nitrogen on one wall of the container?
What is the volume occupied by 1.000 mol of nitrogen gas at a pressure of 2.00 atm and a temperature of 100 K? Gas constant R = 0.08206 L.atm. mol.
According to the ideal gas law, a 0.9054 mol sample of krypton gas in a 1.023 L container at 274.0 K should exert a pressure of 19.90 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. % According to the ideal gas law, a 9.344 mol sample of oxygen gas in a 0.8267 L container at 500.1...
Question 16 10 pts Nitrogen gas (N2) behaves as an ideal gas at normal temperatures. Consider a 5.00L tank filled with 3.50 mol at room temperature (25.0°C). (R = 0.08206 L'atm/mol-K) • What is the pressure of the tank? Pressure atm • The tank is left slightly open and 1.50 moles of the gas escapes. What is the new pressure inside of the tank? (Hint: how much gas is left in the tank?) Pressure atm • The tank has a...
A rigid cylinder (15 cm radius, 15 cm height) contains nitrogen gas (N2) at standard temperature and pressure. What is the total translational kinetic energy of the gas molecules in the cylinder? 2.7 kJ 0.51 kJ 1.6 kJ 0.86 kJ
A gas mixture contains 0.150 mol of oxygen (O2) gas, 0.116mo lof nitrogen (N2) gas. and 0.211 mol of argon (Ar) gas in a 0.500L flask at 298K. What is the partial pressure of N2 the mixture?
A gas mixture contains 0.600 mol of N2, 0.150 mol of H2, and 0.400 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 8.00 L vessel at 27.00°C. A) What is the total pressure in the vessel (atm)? B) What is the pressure (atm) of H2? C) What is the pressure (atm) of N2? D) What is the pressure (atm) of CH4?
A volume of 30.0 mL of nitrogen gas was collected over water at 24.0°C and 0.98 atm. The vapor pressure of water at this temperature is 0.03 atm. a. What is the partial pressure of the nitrogen gas sample, (use Dalton's law)? b. What would the new volume of this gas be at STP. (Use the combined gas law)?
3. A volume of 30.0 mL of nitrogen gas was collected over water at 24.0°C and 0.98 atm. The vapor pressure of water at this temperature is 0.03 atm. a. What is the partial pressure of the nitrogen gas sample, (use Dalton's law)? b. What would the new volume of this gas be at STP. (Use the combined gas law)?