Acompressed cylinder of gas contains 45.6 mol of n2 gas at a pressure of 3.75 x 105 pa and a temperature of 23.6°c. what volume of gas has been released into the atmosphere if the final pressure in the cylinder is 5.67 x 105 pa? assume ideal behavior and that the gas temperature is unchanged.

0.102 Liters

Explanation

According to the ideal gas equation:

P = Pressure of the gas = = 3675 atm     (1 kPa= 0.0098 atm)

V= Volume of the gas = ?

T= Temperature of the gas = 23.6°C = 296.6 K    

R= Gas constant = 0.0821 atmL/K mol

n= moles of gas = 45.6

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

    (At constant temperature and number of moles)

where,

= initial pressure of gas  =

= final pressure of gas  =

= initial volume of gas   = 0.302 L

= final volume of gas  = ?

The final volume has to be 0.199 L, thus (0.302-0.199) L= 0.102 L must  release into the atmosphere.

Therefore the answer is 0.102 L

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