Electrochemistry · Chemistry · VITEEE

4.5 g of aluminium (Atomic mass 27 amu ) is deposited at cathode from $\mathrm{Al}^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from $\mathrm{H}^{+}$ions in the solution by the same quantity of electric charge will be

How long should water be electrolysed by passing through 100 amperes current so that oxygen released can completely burn 27.66 g of diborane? (Weight of $B=10.8 \mathrm{u}$ )

The ionic conductance of following cation in a given concentration are in the order.

Consider the following cell reaction.

$$\begin{aligned} & 2 \mathrm{Fe}(s)+\mathrm{O}_2(g)+4 \mathrm{H}^{+}(a q) \longrightarrow \\ & 2 \mathrm{Fe}^{2+}(a q)+2 \mathrm{H}_2 \mathrm{O}(l), E^{\circ}=1.67 \mathrm{~V} \\ \end{aligned}$$

At $$[\mathrm{Fe}^{2+}]=10^{-5} \mathrm{M}, {\mathrm{P}}{ }_2=3 \mathrm{~atm}$$ and $$\mathrm{pH}=2.5$$, the cell potential at $$25^{\circ} \mathrm{C}$$ is

When an electrolytic solution conducts electricity, the current is carried by

An electrochemical cell has two half cell reactions as,

$$\begin{aligned} A^{2+}+2 e^{-} & \longrightarrow A ; E_{A^{2+} / A}^0=0.34 \mathrm{~V} \\ X & \longrightarrow X^{2+}+2 e^{-} ; E_{X^{2+} / X}^0=-2.37 \mathrm{~V} \end{aligned}$$

The cell voltage will be

Electrolysis of an aqueous solution of sodium ethanoate gives