Question

Question 1 a sample of 0.255 mole of gas has a volume of 748 ml at 28°c. calculate the pressure of this gas. (r= 0.0821 l ∙ atm / mol ∙ k) 0.784 atm 8.42 atm 0.00842 atm 7.84 × 10-4 atm none of the above

Answer 1

The correct answer to this complex question is 8.428 atm.

Answer 2

Answer : The pressure of the gas is, 8.42 atm

Explanation :

Using ideal gas equation,

`PV=nRT`

where,

P = pressure of the gas = ?

V = volume of the gas = 748 ml = 0.748 L

conversion used : (1 L = 1000 ml)

T = temperature of the gas =
`28^oC+273+28=301K`

n = number of moles of the gas = 0.255 mole

R = gas constant = 0.0821 L.atm/mole.K

Now put all the given values in the ideal gas equation, we get the pressure of the gas.

`P* (0.748L)=0.255mole* (0.0821L.atm/mole.K)* (301K)`

`P=8.42atm`

Therefore, the pressure of the gas is, 8.42 atm