Question

Calculate the amount of 50% H2SO4 required to decompose 25g of Marble ?

Answer 1

Here is the reaction for the question:

H2SO4 + CaCO3 -----> CaSO4 +H2O + CO2

To answer this question, we will calculate the moles and find mole ratio:

Mole ratio of H2SO4: CaCO3  =  1:1

Moles of the CaCO3  -       molar mass (40+12+48=100)
= mass/molar mass  =25/100
                                  =0.25 moles
since mole ratio is 1:1 then moles of H2SO4 required will also be 0.25moles

This equation is for 100% H2SO4, hence moles of 50 % H2SO4 required is :   100=0.25
         50  =0.25x100/50 =  0.5 moles (twice as much is needed)
Therefore mass required = molesx molar mass
                                           = 0.5 x 100 =50g

Therefore the mass required of the 50% H2SO4 is 50 grams

Answer 2

ANSWER:

B (49gm)

Solution :

CaCO3(100g) + H2SO4(98g) → CaSo4+ H2O+ CO2

100g CaCO3 require 98gm H2SO4

25g CaCO3 require =  98100×25gm  pureH2SO4

                                  =24.5gpureH2SO4

Hence, wt 50% pure H2SO4 will be 49 gm (24.5*100/50)

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