During discharging of lead-storage acid battery following reaction takes place:
`Pb(S)+PbO_(2)(S)+2H_(2)SO_(4)`
`rarr2PbSO_(4)(S)+2H_(2)O`
If `2.5` amp of current is drawn for 965 minutes, `H_(2)SO_(4)` consumed is :

Options

A. `0.75` mol
B. `3.00` mol
C. `1.50` mol
D. `4.50` mol

Answer

C

Explanation

Oxidation :
`Pb(s)+4H^(+)(Aq)+SO_(4)^(2-)(aq)+2e^(-)`
Reduction :
`PbO_(2)(s)+4H^(+)(aq)+S_(4)^(2-)(aq)+2E^(-)rarrPbSO_(4)(s)+2H_(2)O(l)`
During discharging `H_(2)SO_(4)` consumed
W = zit
Mass of `H_(2)SO_(2)=2mol=2xx98g`
`w=(2xx98xx2.5xx965xx60)/(2xx96500)=147g=1.5mol`