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?
Calculating pressure using the ideal gas equation:
Now, Volume of the container = 2L =
where, a = length of the side of the container
Area of one side of the container =
Force exerted on one wall of the container =
Pressure is divided by because a cubic container has walls.
A cubic container of volume 2.00 L holds 0.500 mol of nitrogen gas at a temperature...
A cubic container of volume 1.77 L holds 0.550 mol of nitrogen gas at a temperature of 26°C. What is the net force due to the nitrogen on one wall of the container (in N)? (Enter the magnitude.) Compare the magnitude of this force to the sample's weight.
A sample of nitrogen gas contains 5.0 mol in a volume of 3.5 L. Calculate the new volume of the container if the pressure and temperature are kept constant but the number of moles of nitrogen is changed to 1.4 mol
1.) Use the ideal gas law to calculate the volume occupied by 0.500 mol of nitrogen gas at 1.60 atm pressure and at 27°C. R = 0.0821 L*atm/(K*mol). 0.694 L 7.10 L 7.70 L 7.89 L (separate question) 2.What will be the final gas temperature in kelvins?
A sealed container holds 0.020 moles of ideal nitrogen (N2) gas at a pressure of 1.5 atmospheres and a temperature of 290 K. The atomic mass of nitrogen is 14.0 g/mol. What is the approximate quantity of heat, transferred at constant volume, that raises the temperature of the gas to 300 K, in SI units?
If a 5.00 L container holds 1.56 mol of Ar at a temperature of 290 K, what pressure of Ar gas would you expect? If a 5.00 L container hold 1.56 mol of Ar at a temperature of 290 K, what pressure of Ar gas would you expect?
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.
2. A sample nitrogen gas has a volume of 1.00 L at STP. What is the temperature in °C if the volume is 10.0L at 2.00 atm?
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 each side, at 1.50 atm of pressure, what is the rms speed of the nitrogen molecules?
A flexible container at an initial volume of 6.13 L contains 4.51 mol of gas. More gas is then added to the container until it reaches a final volume of 16.7 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container. number of moles of gas: _______ mol