The reaction taking place in a galvanic cell is as given

$$\mathrm{A}(\mathrm{s})+\mathrm{B}^{2+}\left(\mathbf{1} \mathbf{1} \mathbf{1 0} \mathbf{0}^{-\mathrm{M}} \mathbf{M}\right) \rightarrow \mathrm{B}_{(\mathrm{s})}+\mathrm{A}^{2+}(0.1 \mathrm{M}).$$

The emf of the cell is $$+2.651 \mathrm{~V}$$. If the standard emf of the cell is $$+2.71 \mathrm{~V}$$, what is the value of $$\mathrm{X}$$ ?

What will be the emf of the following cell at 25$$^\circ$$C?

Fe/Fe$$^{2+}$$ (0.001 M) | | H$$^+$$ (0.01 M) | H$$_2$$(g) (1 Bar) | Pt(s)

$$E_{(F{e^{2+}} /Fe)}^o = - 0.44$$ V; $$E_{({H^ + }/{H_2})}^o = - 0.00$$ V

Calculate the molar conductance of 0.025 M aqueous solution of calcium chloride at 25$$^\circ$$C. The specific conductance of calcium chloride is 12.04 $$\times$$ 10$$^{-2}$$ Sm$$^{-1}$$

Given that molar conductances for Ba(OH)$$_2$$, BaCl$$_2$$ and NH$$_4$$Cl are 523.28, 280.0 and 129.8 $$\Omega^{-1}$$ cm$$^2$$ mol$$^{-1}$$ respectively. What is the molar conductivity ($$\Omega^{-1}$$ cm$$^2$$ mol$$^{-1}$$) of NH$$_4$$OH?