Electrolysis of fused NaCl will give

• Na

• NaOH

• NaClO

• NaClO₃

How long it will take to deposit 1.0 g of chromium when a current of 1.25 A flows through a solution of chromium (III) sulphate ? (Molar mass of Cr = 52)

• 1.24 min

• 1.24 h

• 1.24 s

• None of these

The compounds formed at anode in the electrolysis of an aqueous solution of potassium acetate, are

• C₂H₆ and CO₂

• C₂H₄ and CO₂

• CH₄ and H₂

• CH₄ and CO₂

What is the electrode potential (in V) of the following electrode at 25°C ?

Ni²⁺ (0.1 M) | Ni(s)

(Standard reaction potential of Ni²⁺ | Ni is -0.25V, $\frac{2.303 \mathrm{RT}}{\mathrm{F}} = 0.06$)

• -0.28V

• -0.34V

• -0.82V

• -0.22V

EMF or hydrogen electrode in terms of pH at 1 atm pressure is

• E_{H2 = $\frac{\mathrm{RT}}{\mathrm{F}}\mathrm{pH}$}

• E_{H2 = $\frac{\mathrm{RT}}{\mathrm{F}}\frac{1}{\mathrm{pH}}$}

• E_{H2 = $\frac{2.303 \mathrm{RT}}{\mathrm{F}}\mathrm{pH}$}

• E_{H2 = -0.0591 pH}

Assuming that constant current is delivered. How many kW-h of electricity can be produced by the reaction of 1.0 mole Zn with Cu ion in a Daniel cell in which all the concentration remains 1.00 M.

(Given E$\mathrm{Given} \mathrm{E}{°}_{\mathrm{Zn}/{\mathrm{Zn}}^{+}=0.76}$=0.76V),

• 0.069 kW-h

• 0.074 kW-h

• 0.080 kW-h

• 0.059 kW-h

What amount of Cl₂ gas liberated at anode, if 1 ampere current is passed for 30 minute from NaCl solution ?

• 0.66 mol

• 0.33 mol

• 0.66 g

• 0.33 g

$$\begin{gathered} \mathrm{For} \mathrm{the} \mathrm{given}, \\ \mathrm{Sn}\to {\mathrm{Sn}}^{2+ }(0.1 \mathrm{M}) + 2\mathrm{e} \\ (\mathrm{Given} {\mathrm{E}}_{\mathrm{Sn}/{\mathrm{Sn}}^{2+}}^0= 0.136 \mathrm{V}) \\ \mathrm{The} \mathrm{electrode} \mathrm{potential} \mathrm{of} \mathrm{the} \mathrm{cell} \mathrm{at} 25° \mathrm{C} \mathrm{is}: \end{gathered}$$

• 0.165 V

• 0750 V

• 0.421 V

• 0.012 V

A 35% solution LiCl was electrolysed by using a 2.5A current for 0.8h.Assuming thecurrent efficiency of 90%. The mass of LiOHproduced at the end of electrolysis.
[Atomic mass of Li=7] is:

• 1.61 g

• 2.71 g

• 4.02 g

• 3.70 g

Which of the following formula is applicable for weak electrolyte:

• $\mathrm{\alpha }=\frac{{\mathrm{\lambda }}_{\mathrm{m}}}{{\mathrm{\lambda }}_{\mathrm{m}}^{\circ }}$

• ${\mathrm{K}}_{\mathrm{a}}=\frac{{\mathrm{C\alpha }}^2}{(1-\mathrm{\alpha })}$

• ${\mathrm{K}}_{\mathrm{a}}=\frac{{\mathrm{C\lambda }}_{\mathrm{m}}^2}{{\mathrm{\lambda }}_{\mathrm{m}}^{\circ }({\mathrm{\lambda }}_{\mathrm{m}}^{\circ }-{\mathrm{\lambda }}_{\mathrm{m}})}$

• All of these