Question

A 10​-liter ​[l] flask contains 1.4 moles​ [mol] of an ideal gas at a temperature of 20 degrees celsius ​[degrees​c]. What is the pressure in the flask in units of atmospheres​ [atm]?

Answer 1

Step-by-step explanation:

The given data is as follows.

P = ?, V = 10 liter

n = 1.4 moles, T =
`20^(o)C` = (20 + 273) K = 293 K

As per the ideal gas equation, PV = nRT. Therefore, putting the given values into the formula as follows.

PV = nRT

`P * 10 L = 1.4 mol * 0.0821 Latm/mol K * 293 K`

P = 3.36 atm

= 3.4 atm (approx)

Thus, we can conclude that the pressure in the flask in units of atmospheres​ is 3.4 atm.

Answer 2

The pressure in the flask is 3.4 atm.

pV = nRT

T = (20 + 273.15) K = 293.15 K

p = (nRT)/V = (1.4 mol × 0.082 06 L·atm·K⁻¹mol⁻¹ × 293.15 K)/10 L = 3.4 atm