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Vinil7 [7]
3 years ago
7

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 th

e pressure in the flask in units of atmospheres​ [atm]?
Chemistry
2 answers:
Lynna [10]3 years ago
4 0

The pressure in the flask is 3.4 atm.

<em>pV</em> = <em>nRT </em>

<em>T</em> = (20 + 273.15) K = 293.15 K

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

WARRIOR [948]3 years ago
3 0

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 \times 10 L = 1.4 mol \times 0.0821 Latm/mol K \times 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.

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