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Question

If excess water is added into a 100 g bottle sample labelled as "112% H2SO4" and is reacted with 5.3 g Na2CO3, then find the volume of CO2 evolved at STP after the completion of the reaction : [R=0.0821 L atm mol1 K1]
H2SO4+Na2CO3Na2SO4+H2O+CO2
  1. 2.46 L
  2. 24.6 L
  3. 1.12 L
  4. 11.2 L


Solution

The correct option is C 1.12 L
Balanced chemical reaction :
H2SO4+Na2CO3Na2SO4+H2O+CO2

Moles = Given massMolar mass
Moles of Na2CO3 = 5.3106=0.05 mol
Moles of H2SO4 = 11298=1.14 mol
For limiting reagent = MolesStochiometric coefficent
For Na2CO3 = 0.051=0.05
For H2SO4 = 11298=1.14.
The ratio for Na2CO3 is less hence it is a limiting reagent.
According to stoichiometric coefficient : 
Moles of CO2 formed = Moles of Na2CO3 reacted = 0.05 mol.
Volume of CO2 evolved at STP conditions = 0.05×22.4=1.12 L

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