What mass will 2.5 L of chlorine gas be at STP?

m = 7.7 g Cl2

Explanation: To find mass of chlorine gas we will first derive the ideal gas law formula and find first the number of moles of Cl2. At STP, Pressure is equal to 1 atm and temperature is 273 K.

n= PV /RT

= 1 atm ( 2.5 L) /0.0821 L.atm / mole.K ( 273 K)

= 0.11 mole Cl2

Convert moles of Cl2 to grams using the molar mass of Cl2 which is 70 g Cl2.

0.11 mole Cl2 x 70 g Cl2 / 1 mole Cl2

= 7.7 g Cl2

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.