Question

5. A 4.44 L container holds 0.481 mol of O2 at 22.6°C. What is the pressure of the tank?

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Answer 1

Answer: The pressure of given tank is 2.63 K.

Step-by-step explanation:

The given data is as follows.

V = 4.44 L, n (no. of moles) = 0.481 mol,

T =
`22.6^(o)C` = (22.6 + 273) K = 295.6 K

R (ideal gas constant) = 0.0821 atm L/mol K

Now, using the ideal gas equation we will calculate the pressure of the given tank as follows.

PV = nRT

`P * 4.44 L = 0.481 mol * 0.0821 atm L/mol K * 295.6 K`

P = 2.63 atm

Therefore, we can conclude that the pressure of given tank is 2.63 K.

Answer 2

Answer: The pressure of the tank will be 2.63 atm

Step-by-step explanation:

According to ideal gas equation:

`PV=nRT`

P = pressure of gas = ?

V = Volume of gas = 4.44 L

n = number of moles = 0.481

R = gas constant =
`0.0821Latm/Kmol`

T =temperature =
`22.6^0C=(22.6+273)K=295.6K`

`P=(nRT)/(V)`

`P=(0.481mol* 0.0821Latm/K mol* 295.6K)/(4.44L)=2.63atm`

The pressure of the tank will be 2.63 atm