If 65.0 L of oxygen at 19.0 ∘C and an absolute pressure of 2.35 atm are...

If 65.0 L of oxygen at 19.0 ∘C and an absolute pressure of 2.35 atm are compressed to 49.6 L and at the same time the temperature is raised to 58.5 ∘C, what will the new pressure be?

Expert Solution

genius_generous answered 8 months ago

A 27.5 L sample of oxygen gas is at 25°C and 1.05 atm. If the gas...

A 27.5 L sample of oxygen gas is at 25°C and 1.05 atm. If the gas is cooled to – 40.°C while the pressure is increased to 2.00 atm, calculate the new volume of the gas. Can u please show with dymentional analysis?

If the total pressure is 1.07 atm, what is the partial pressure of Oxygen?

1.) Gas Number of moles N2 3.10 O2 0.76 CO2 0.12 If the total pressure is 1.07 atm, what is the partial pressure of Oxygen? (Your answer will be in atmospheres, but do NOT include units - Blackboard won't allow them. Use two decimal places, and simply give the number portion.) 2.) A reaction is carried out that produces hydrogen gas. The gas is collected in an inverted beaker over water at 25 oC. The vapor pressure of water at...

A sample of oxygen gas occupies a volume of 9.30 L at 52.0°C and 0.790 atm....

A sample of oxygen gas occupies a volume of 9.30 L at 52.0°C and 0.790 atm. If it is desired to increase the volume of the gas sample to 11.0 L, while decreasing its pressure to 0.569 atm, the temperature of the gas sample at the new volume and pressure must be °C.

A sample of O2 gas has a volume of 19.0 L at a pressure of 1.50...

A sample of O2 gas has a volume of 19.0 L at a pressure of 1.50 atm and a temperature of 23 °C. What volume, in liters, will the gas occupy at 3.50 atm and 271 °C? Assume ideal behavior

What is the pressure in a 5.00 L tank with 9.40 moles of oxygen at 39.3 °C?

What is the pressure in a 5.00 L tank with 9.40 moles of oxygen at 39.3 °C? A balloon at 30.0°C has a volume of 222 mL. If the temperature is increased to 58.1°C and the pressure remains constant, what will the new volume be, in ml?

2.35 kg of oxygen as an ideal gas at 4.00 bar and 400 ° C develop...

2.35 kg of oxygen as an ideal gas at 4.00 bar and 400 ° C develop an adiabatic process up to a pressure of 0.200 bar. What is the work in kJ, done during this process?

Knowing that at 0 oC and an oxygen pressure of 1.00 atm, the aqueous solubility of...

Knowing that at 0 oC and an oxygen pressure of 1.00 atm, the aqueous solubility of O2 (g) is 48.9 mL O2 per liter. The approximate values for the molarity of O2 (g) in solution and the partial pressure of O2 above a 8.23 x 10-4 M O2 (g) saturated aqueous solution at 0 oC are respectively: A. 2.18 M and 3.78 x 10-4 atm B. 2.18 x 10-3 M and 0.378 atm C. 0.0446 M and 0.0179 atm D....

A 5.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure. What is the final...

A 5.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure. What is the final pressure in the flask if an additional 2.00 g of N2 gas is added to the flask and the flask cooled to -55°C? a.) 0.987 atm b.) 1.35 atm c.) 1.84 atm d.) 0.255 atm

The concentration of oxygen inside a 5000 L tank at 1 atm is to reduced by...

The concentration of oxygen inside a 5000 L tank at 1 atm is to reduced by pressure purging prior to charging a fuel into the tank. The tank is charged with nitrogen up to a high pressure and then vented down to atmospheric pressure. If the process is repeated, the concentation of the oxygen will decrease. It is possible to do this many times in order to ultimately reach desired concentration. You can assume that a fully charge tank contains...

If 1.00 mol of argon is placed in a 0.500-L container at 19.0 ∘C , what...

If 1.00 mol of argon is placed in a 0.500-L container at 19.0 ∘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.

Question