Question

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

Answer 1

Answer:  The pressure of the tank will be 2.63 atm

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 =$22.6^0C=(22.6+273)K=295.6K$

$P=\frac{nRT}{V}$

$P=\frac{0.481mol\times 0.0821Latm/K mol\times 295.6K}{4.44L}=2.63atm$

The pressure of the tank will be 2.63 atm

Answer 2

Answer: The pressure of given tank is 2.63 K.

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

 $P \times 4.44 L = 0.481 mol \times 0.0821 atm L/mol K \times 295.6 K$

              P = 2.63 atm

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