Question

Consider the following unbalanced equation for a redox reaction that occurs in acidic solution:

BrO₄^-+ Si → BrO₃^- + SiO₂

When the equation is balanced, the ratio

(number of moles of BrO₄^-) / (number of moles of Si) is equal to

• A. 1/3
• B. 1/2
• C. 3/1
• D. 3/2

• E. 2/1

Answer 1

BALANACING IN ACIDIC MEDIUM:

i. Balance the metal first

ii. Balance oxygen atom by adding H2O on that side in which it has less number of oxygen atom

iii. To balance hydrogen atom, add twice H+ on the other side of H2O added in above step

iv. Balance charge by adding e- on required side

Reduction half rection:

------>(a)

Oxidation half reaction:

-------->(b)

Now, 2(a)+(b)=>

Number of moles of / number of moles of Si =2/1

Answer is (E)