Question
Question: In transforming \[0.01~\] mole of \[~PbS~\] to \[PbS{{O}_{4}},\] the volume of \(10\) volume \[H_{2}...
In transforming 0.01 mole of PbS to PbSO4, the volume of 10 volume H2O2 required will be:
A. 11.2mL
B. 22.4mL
C. 33.6mL
D. 44.8mL
Solution
To solve this question we should always learn the properties of the hydrogen peroxide. Hydrogen peroxide has oxidizing and reducing nature. It behaves as an oxidising as well as reducing agent in the both acidic and alkaline mediums.it is a powerful oxidising agent but a weak reducing agent.
Complete step by step answer:
As in the given question we have to give the product of the following reactant: H2O2 and PbS
On mixing the both reactants we get some output from the reaction. We all know that aqueous solution of hydrogen peroxide oxidises the lead sulphide into lead sulphate As in the given below reaction we can see: H2O2 →H2O+[O]
From the above given reaction we can say that hydrogen peroxide gives one nascent oxygen. Now this nascent oxygen will oxidise the lead sulphide. We can see the oxidation of the lead sulphide as given below: PbS+4[O]→PbSO4
So, after getting the product from the reaction we can say that by reacting hydrogen peroxide with lead sulphide we get the white product of the lead sulphate.
PbS+4H2O2→PbSO4+4H2O
0.04 mol of H2O2 is required to react with 0.01mol PbS
Molarity of H2O2 may be calculated as,
Volume strength =Molarity×11.2
⇒10=M×11.2
⇒M=0.892
Thus, Number of moles =1000MV
0.04=10000.892×V
⇒V=44.8mL
So, the correct answer is Option D.
Note: Properties of Pure anhydrous hydrogen peroxide is a syrupy liquid. It is colourless but gives a bluish tinged in thick layers. It is odourless. Its specific gravity is 1.45 at and more viscous than water. This is due to the fact that molecules are more associated through H bonding. It is soluble in water, alcohol, and ether in all proportions. It has a bitter taste. It is injurious to skin.