Some fuel cells are used to produce energy from the combination of hydrogen and
oxygen. The half-equations for a hydrogen-oxygen fuel cell in alkaline solution are:
2H2O(l) + 2e– ---> H2(g) + 2OH–(aq)
E cell : –0.83 V
½O2(g) + H2O(l) + 2e– ----> 2OH–(aq)
E cell : + 0.4 V
a) The equation for the cell reaction is
A.) 3H2O(l) + ½O2 ----> H2(g) + 4OH–(aq)
B.) H2(g) + 4OH– ----> 2O(l) + ½O2(g)
C.) H2(g) + ½O2 -----> 2O(l)
D.) H2 ---> H2(g) + ½O2(g)
And answer is C anyone can explain to me how and what is going on?
Oh and also in the next question itself they ask about the E cell Value the thing is I know the formula which is E cell: (Right Hand electrode) - (Left hand Electrode)
But In equations I can't seem to recognize which is right and which one is left
I already kinda bit wobbly on this chapter :'(