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?

Solutions

Expert Solution

genius_generous answered 1 month ago

Next > < Previous

Related Solutions

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?

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.

A 1.100−L flask at 25∘C and 1.00 atm pressure contains CO2(g) in contact with 100.0 mL...

A 1.100−L flask at 25∘C and 1.00 atm pressure contains CO2(g) in contact with 100.0 mL of a saturated aqueous solution in which [CO2(aq)] = 3.29×10−2 M. a) What is the value of Kc at 25∘C for the equilibrium CO2(g)⇌CO2(aq) Answer: Kc = 0.804 b) If 0.01400 M of radioactive 14CO2 is added to the flask, how many moles of the 14CO2 will be found in the gas phase and in the aqueous solution when equilibrium is reestablished? [Hint: The radioactive 14CO2 distributes itself between the two phases in exactly the same...

A 83.0 L cylinder containing C2H4F2 at a pressure of 3.00 atm is connected by a...

A 83.0 L cylinder containing C2H4F2 at a pressure of 3.00 atm is connected by a valve to 44.0 L cylinder containing PF5 at 5320 torr pressure. Calculate the partial pressure (atm) of PF5 when the valve is opened.

Subjects