Electrochemistr...

For an electrochemical reaction occuring in a galvanic cell.
$$2{ Fe }_{ \left( aq \right)  }^{ +3 }+{ Zn }_{ \left( s \right)  }\rightarrow { Zn }_{ \left( aq \right)  }^{ +2 }+2{ Fe }_{ \left( aq \right)  }^{ +2 }$$
if concentration of $${ Fe }^{ +2 }$$ is increased.

The approximate time duration in hours to electroplate $$30\space g$$ of calcium from molten calcium chloride using a current of $$5 \space A$$ is (At. mass of $$Ca = 40g/mol$$)

Consider the following equations for a cell reaction :
$$A  + B \rightarrow C + D \,; E^o = x \,volt, \Delta G = \Delta G_1$$
$$2A  +2 B \rightarrow 2C +2D \,; E^o = x \,volt, \Delta G = \Delta G_2$$

In which of the following conditions is the potential for the following half-cell reaction maximum?
$$2H^+ + 2e^{-} \longrightarrow H_2$$

Given that $$E^o_{Ag^+/Ag} = + 0.8V$$ and $$ E^o_{Ni^{+2}/Ni} = 0.25 V$$. Which of the following statement is true with regard to this?

Which of the following statements about the spontaneous reaction occurring in a galvanic cell is always true?

What is the amount of chlorine evolved, when 2A of current is passed for 30 minutes in an aqueous solution of NaCl?

Which of the following does not evolve oxygen at anodes when electrolysis is carried?

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reaction and their standard potential are given below:

If $$9$$ gm $$H_2O$$ is electrolysed completely with the current of $$50\%$$ efficiency then?