Question

1. How many grams of H2O2, are required to convert
0.1mole PbS to 0.1mole PbSO4 ? [AIPMT, 2002)
(A) 12.8 g
B) 13.6 g
(C) 16 g
(D) 3.4 g​

Answer 1

Explanation:

Solution :

The reaction is

4H2O2+PbS→4H2O+PbSO4

Thus 0.01 mole PbS reacts with 0.01∗4i.e. 0.04 moles of H2O2

Thus volume of H2O2 needed

=0.04∗11.2/10=0.0448Lor44.8mL

 

Answer 2

The correct answer is option B.

Explanation:

$PbS+4H_2O_2\rightarrow PbSO_4+4H_2O$

According to reaction,4 mole of hydrogen peroxide is used to covert 1 mole of  lead(II) sulfide to 1 mole of lead(II) sulfate.

Then to convert 0.1 mole of lead (II) sulfide we will need:

$\frac{4}{1}\times 0.1mol=0.4 mol$ of hydrogen peroxide

Mass of 0.4 moles of hydrogen peroxide:

0.4 mol × 34 g/mol =  13.6 g

The correct answer is option B.

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