Chlorine is widely used to purify municipal water supplies and to treat swimming pool water. suppose that the volume of a particular sample of cl2 gas is 8.80 l at 895 torr and 24 °c
1. how many grams of cl2 are in the sample? 2.what volume will the cl2 occupy at stp? 3.at what temperature will the volume be 15.00 l if the pressure is 875 torr? 4.at what pressure will the volume equal 6.40 l if the temperature is 58 ? c?

1.mass of Cl in sample = 15.09g

2.volume at STP= 9.53L

3.Temperature at 15L and 875torr= 494.7K

4.pressure at 6.4L and 58 °C= 1.80542atm

Explanation:

(1.) Using the ideal gas law to calculate, PV=nRT

R= 0.08206Latm/mol/K

we will convert P from torr to atm and T from  °C to K

P=895torr = 895/760 =1.1776atm

T= 24 °C+273 = 297K

n =

n=

n= 0.425 mol

mass= n*molar mass

molar mass of Cl = 35.5g/mol

mass= 0.425 *35.5

mass of Cl in sample = 15.09g

(2.) At stp, T=273K, P=1atm.

  Using the combined gas law ,

v1 = 8.8L, p1= 1.1776atm, t1= 297K, v2=?, p2= 1atm, t2=273K

v2=9.53L

(3.) t1=?  v1=15L   p1= 875torr/760 = 1.1513atm,

t1= 494.7K

(4.) p1=?  v1=6.4L t1= 58°C+273 =331K

p1= 1.80542atm

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