A) \[2{{H}_{2}}(g)+{{O}_{2}}(g)\to 2{{H}_{2}}O(l)\]
B) \[2Fe(s)+{{O}_{2}}(g)+4{{H}^{+}}(aq)\to \] \[2F{{e}^{2+}}(aq)+2{{H}_{2}}O(l)\]
C) \[Pb(s)+Pb{{O}_{2}}(s)+2{{H}_{2}}S{{O}_{4}}(aq)\to \] \[2PbS{{O}_{4}}(s)+{{H}_{2}}O(l)\]
D) \[Cd(s)+2Ni{{(OH)}_{3}}(s)\to \] \[CdO(s)+2Ni{{(OH)}_{2}}+2{{H}_{2}}O(l)\]
Correct Answer: A
Solution :
Galvanic cells which use energy of combustion of fuels like \[{{H}_{2}},C{{H}_{4}},C{{H}_{3}}OH\]etc, as the source to produce electronic energy are called fuel cells. \[2{{H}_{2}}(g)+{{O}_{2}}(g)\to 2{{h}_{2}}O(l)\]
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