Electrolytic Cells and Electrolysis

What amount of silver will be deposited by passing $2\mathrm{F}$ electricity through two solutions containing $0.1 \mathrm{M} {\mathrm{AgNO}}_3$ and $0.2 \mathrm{M} {\mathrm{AgNO}}_3$.

The image below shows electrolysis of an electrolyte using a DC voltage source.

Based on this, Which of the following statements is/are correct?

(i) The solution remains electrically neutral during electrolysis.

(ii) Electrons flow from the current source towards the solution at one electrode, and an equal number of electrons flow away from the solution at the other electrode.

(iii) The number of positive ions moving towards one electrode is always equal to the number of negative ions moving towards the other electrode.

Write a anodic reaction involved in the electrolysis of brine solution using mercury electrode.

Write the reactions that occur on anode and cathode during electrolysis of dilute sulphuric acid.

The product obtained at cathode during electrolysis of dilute sulphuric acid is:

The product obtained at cathode during electrolysis of dilute sulphuric acid is hydrogen gas.

The product obtained at anode during electrolysis of dilute sulphuric acid is hydrogen gas.

Electrolysis of $\mathrm{NaCl}$ solution gives _____ at anode. (chlorine / oxygen)

A sample of ${\mathrm{Al}}_2{\mathrm{O}}_3$, dissolved in a molten fluoride bath, is electrolysed using a current of $1.20 \mathrm{A}.$ What is the rate of production of $\mathrm{Al}$ in $\mathrm{gram}/\mathrm{hour}$ ?

Give your answer by multiplying with 1000 and rounding off to three significant figures.

A solution containing $\mathrm{Cu}\left(\mathrm{I}\right), \mathrm{Ni}$ and $\mathrm{Zn}$ cyanide complexes was electrolysed and a deposit of $0.175 \mathrm{g}$ was obtained. The deposit contained $72.8\% \mathrm{Cu}, 4.3\%\mathrm{Ni}$ and $22.9\%$ $\mathrm{Zn}$. No other element was released. Calculate the number of coulombs passed through the solution. (At. wt. $\mathrm{Cu} = 63.5, \mathrm{Zn} = 65, \mathrm{Ni} = 59$ )

Report the answer by rounding off to three significant figures

If $40 \mathrm{mL}$ of $0.125 \mathrm{M}$ of ${\mathrm{NiSO}}_4$ solution is electrolysed by a current of $0.05 \mathrm{amp}$ for $40 \mathrm{minutes}$,

 The number of grams of the product deposited at the cathode is $Q X {10}^{-3}$, Report the value of $Q in 2$ significant figures.

$\left(\mathrm{Consider},1\mathrm{F}=96500 \mathrm{coulomb} \mathrm{and} \mathrm{atomic} \mathrm{weight} \mathrm{of} \mathrm{Ni} \mathrm{is} 58.7\mathrm{g}\right)$

Lake Cayuga has a volume of water estimated to be $8.2\times {10}^{12}$ $\mathrm{L}$. A power station not so far above Cayuga's waters produces electricity at the rate of $1.5\times {10}^6$ $\mathrm{coulombs}$ $\mathrm{per} \mathrm{second}$ at an appropriate voltage. How long(in years) would it take to electrolyse the lake?

If the answer is $\mathrm{X}\times {10}^4. \text{Give the value of} \mathrm{X}?$

How long (in sec) should a current of $0.5 \mathrm{amp}$ be passed through $50 \mathrm{mL}$ of a $0.10 \mathrm{M} \mathrm{NaCl}$ solution in order to make its $\mathrm{pH}=12$, assuming that no volume changes?

Round-off the answer to the nearest integer.

One hundred millilitres of$0.8 \mathrm{M}$ copper sulphate solution is electrolysed for $30$minutes by passing a current of $5 \mathrm{amp}$. Calculate the amount of copper sulphate in grams in the solution.

Round off answer to the nearest integer value.

Electric current is passed through two cells $\text{'}\mathrm{A}\text{'}$ $\text{'}\mathrm{B}\text{'}$ in series. Cell$\text{'}\mathrm{A}\text{'}$ contains an aqueous solution of ${\mathrm{Ag}}_2{\mathrm{SO}}_4$ and platinum electrodes. The cell  $\text{'}\mathrm{B}\text{'}$ contains an aqueous solution of ${\mathrm{CuSO}}_4$ and $\mathrm{Cu}$ electrodes. The current is passed till $1.6 \mathrm{g}$ of oxygen is liberated at the anode of cell $\text{'}\mathrm{A}\text{'}.$

Calculate the mass of silver deposited(in grams) at the cathodes $(\mathrm{Ag}=108, \mathrm{Cu}=63.5)$ (Round off answer to the nearest integer value).

For the electrolytic production of ${\mathrm{NaClO}}_4$ from ${\mathrm{NaClO}}_3$ as per reaction:

${\mathrm{ClO}}_3^{-}+{\mathrm{H}}_2\mathrm{O}\to {\mathrm{ClO}}_4^{-}+2{\mathrm{H}}^{+}+2e^{-}$

How many faradays of electricity would be required to produce $1 \mathrm{mole}$ of ${\mathrm{NaClO}}_3$ ?

$50 \mathrm{mL}$ of a $0.1 \mathrm{M} {\mathrm{CuSO}}_4$ solution is electrolysed for $12 \mathrm{minutes}$ at a current of $0.06 \mathrm{amp}$. If $\mathrm{Cu}$ is produced at one electrode and ${\mathrm{O}}_2$ at the other, what will be the $\mathrm{pH}$ of the final solution? For ${\mathrm{HSO}}_4^{-}={\mathrm{H}}^{+}+{\mathrm{SO}}_4^{2-}, {\mathrm{K}}_{\text{diss }}=1·3\times {10}^{-2}$,

Report your answer by multiplying the P^H value obtained in to 10 and rounding off the value to two significant figures.

How many hours are required for a current of $3 \mathrm{amp}$ to decompose electrolytically $18 \mathrm{g}$ of water? 

Express your answer by rounding off the value to two significant figures.

During the electrolysis of aqueous solution of ${\mathrm{CuSO}}_4$ by using platinum electrodes _____ will deposit at cathode.(Copper/Oxygen)

During electrolysis of a solution of $\mathrm{A}\mathrm{g}\mathrm{N}{\mathrm{O}}_3$, $9650$ coulombs of charge is passed through the solution. The mass of silver deposited on the cathode is _____ $\mathrm{g}$.