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------------------------------------------------ 2,500 liters of oxygen gas is produced at 1.00 atm of pressure. It is to be compressed and stored in a 20.0-liter cylinder. If the temperature is constant, calculate the pressure of the oxygen in the cylinder.

A. 125 atm
B. 80.0 atm
C. 8.00 atm
D. 4.00 atm

The pressure of the oxygen in the cylinder can be calculated using the ideal gas law PV = nRT. Therefore, the pressure of the oxygen in the cylinder will be 125 atm.

As we know that,

PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant and T is the temperature (assumed constant). We can also use the proportionality relationship between the initial and final pressures and volumes, P1V1 = P2V2.

Given:

V1 = 2500 L

P1 = 1.00 atm

V2 = 20.0 L

We can rearrange the proportionality equation to find P2:

P2 = P1 * V1/V2

So P2 = 1.00 atm * 2500 L / 20.0 L = 125 atm

Therefore, the pressure of the oxygen in the cylinder will be 125 atm.

It is important to note that compressing a gas to such high pressures is not safe and could cause the cylinder to explode. In practice, this process will be done in steps and in controlled conditions.

Learn more about ideal gas law here:

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