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

307.

How much chlorine will be liberated on passing one ampere current for 30 min. through NaCl solution ?

• 0.66 mole

• 0.33 mole

• 0.66 g

• 0.33 g

Three ampere currernt was passed through an aqueous solution of an unknown salt of Pd for 1 h 2.977 g of Pdⁿ⁺ was deposited at cathode.The value of n is:

(given at wf of Pd= 106.4)

• 6

• 5

• 4

• 3

The metal which can displace all other metals from their salt solution among the following is:

• Al

• Zn

• Cu

• Fe

The standard reduction potentials of half reactions are given below:

F₂ (g) + 2e^- $\to$ 2F^- (aq) ; E⁰ = + 2.85 V

Cl₂ (g) + 2e^- $\to$2Cl^- (aq) ; E⁰ = + 1.36 V

Br₂ (g) + 2e^- $\to$2Br^- (aq) ; E⁰ = + 1.06 V

I₂ (g) + 2e^- $\to$ 2I^- (aq) ; E⁰ = + 0.53 V

The strongest oxidising and reducing agents respectively are:

• chlorine and iodine

• fluorine and iodine ion

• chloride and bromine

• bromine and iodine