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

a. the law of proportion states the combination of 2 atoms in a specific ratio to produce multiple compounds such as the given statement of question ‘1st compound contains 88.8 % cu ’ indicates 88.8 g of cu is present along with 11.2 g oxygen in 100 g of compound whereas the statement ‘2st compound contains 79.9 % cu ’ indicates 79.9 g of cu is present along with 20.1 g oxygen in 100 g of compound

1st compound contains 88.8 g cu

for cu

m = 63 g /mol

atomic % = 88.8 /63 = 1.42

for o

m = 16 g /mol

atomic % = 11.2 /16 = 0.7

b. the emperical formula of 1st compound is

cu1.4o0.7

cu2o