question_answer2) Consider the following\[E{}^\circ \]values \[E{{{}^\circ }_{F{{e}^{3+}}/F{{e}^{2+}}}}=+0.77\,V\] \[E{{{}^\circ }_{S{{n}^{2+}}/Sn}}=-0.14\,V\] Under standard conditions the potential for the reaction \[Sn(s)+2F{{e}^{3+}}(aq)\xrightarrow{{}}2F{{e}^{2+}}(aq)\] \[+S{{n}^{2+}}(aq)\]is
question_answer3) The standard emf of a cell, involving one electron change is found to be 0.591 V at\[25{}^\circ C\]. The equilibrium constant of the reaction is \[(F=96500\text{ }C\text{ }mo{{l}^{-1}})\]
question_answer5) In a cell that utilises the reaction, \[Zn(s)+2{{H}^{+}}(aq)\xrightarrow{{}}Z{{n}^{2+}}(aq)+{{H}_{2}}(g)\] addition of\[{{H}_{2}}S{{O}_{4}}\]to cathode compartment, will
A)
lower the E and shift equilibrium to the left
doneclear
B)
lower the E and shift the equilibrium to the right
doneclear
C)
increase the E and shift the equilibrium to the right
doneclear
D)
increase the E and shift the equilibrium to the left
question_answer6) The\[E_{{{M}^{3+}}/{{M}^{2+}}}^{o}\]values for\[Cr,Mn,Fe\]and\[Co\]are\[-0.41+1.57.+0.77\]and\[+1.97\text{ }V\]respectively. For which one of these metals the change in oxidation state from +2 to +3 is easiest?