Electrochemistr...

According to electrochemical theory of corrosion involves:

$$10800C$$ of electricity on passing through the electrolyte solution deposited $$2.977$$ of metal with atomic mass $${ 106.4gmol }^{ -1 }$$ the charge on the metal cation is:

Number of coulombs required to liberate 0.5 mol of $${ O }_{ 2 }$$ is:

If the density of copper is $$8.94 g/{ cm }^{ 3 }$$, the number of faradays required to plate an area $$(10cm\times 10cm)$$ of thickness of $${ 10 }^{ -2 }$$ cm using $${ CuSO }_{ 4 }$$ solution as electrolyte is:

The ratio of volume of $$H_2$$ and $$Cl_2$$ evolved at NTP by electrolysis of aqueous solution of $$HCl$$ is:

How many faradays are needed for reduction of 2.5 moles of $$Cr_2O_7^{2-}$$ into $$Cr^{3+}$$ ?

A current $$9.65$$ ampere is passed through the aqueous solution $$NaCl$$ using suitable electrodes for $$1000\ s$$. The amount of $$NaOH$$ formed during electrolysis is:

The standard electrode potential of the half cells is given below:
$$Zn^{2+}+2e^{-}\rightarrow Zn; E=-0.76 V$$
$$Fe^{2+}+2e^{-}\rightarrow Fe; E=-0.44 V$$
The emf of the cell $$Fe^{2+}=Zn^{-}\rightarrow Zn^{2+}+Fe $$

Amount of charge is required to convert $$17\ g\ H_{2}O_{2}$$ into $$O_{2}$$.

Given,
$$E_{Ag^{+}/Ag}^{\circ}  = +0.80V, E_{Co^{2+}/Co}^{\circ} = -0.28 V, E_{Cu^{2+}/Cu}^{\circ} = +0.34 V, E_{Zn^{2+}/Zn}^{\circ} = -0.76V$$, 
Which metal will corrode to greater extent?