If the number of moles of $\mathrm{Fe}^{2+}$ ions oxidised by one mole of acidified $\mathrm{MnO}_4^{-}$is $x$, the number of moles of $\mathrm{Fe}^{2+}$ ions oxidised by one mole of acidified $\mathrm{Cr}_2 \mathrm{O}_7^{2-}$ is
One mole of an ideal gas at 300 K and 20 atm expands to 2 atm under isothermal and reversible conditions. The work done by the gas is $-x \mathrm{~kJ} \mathrm{~mol}^{-1}$. The value of $x$ is $\left(R=8.3 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$
At 1000 K , the equilibrium constant for the reaction, $\mathrm{CO}_2(\mathrm{~g})+\mathrm{H}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g})$ is 0.53 . In a one litre vessel, at equilibrium the mixture contains 0.25 mole of $\mathrm{CO}, 0.5$ mole of $\mathrm{CO}_2, 0.6$ mole of $\mathrm{H}_2$ and $x$ moles of $\mathrm{H}_2 \mathrm{O}$. The value of $x$ is
$$ \text { Match the following. } $$
| $$ \text { List I (Reactions) } $$ |
$$ \text { List II (Methods) } $$ |
||
|---|---|---|---|
| (A) | $$ \begin{aligned} \mathrm{Mg}\left(\mathrm{HCO}_3\right)_2 \longrightarrow \mathrm{Mg}(\mathrm{OH})_2 \downarrow & +2 \mathrm{CO}_2 \uparrow \end{aligned} $$ |
(I) | Clark's method |
| (B) | $$ \begin{array}{r} M^{2+}+\mathrm{Na}_4 \mathrm{P}_6 \mathrm{O}_{18}^{2-} \longrightarrow\left[\mathrm{Na}_2 \mathrm{MP}_6 \mathrm{O}_{18}\right]^{2-} +2 \mathrm{Na}^{+} \end{array} $$ |
(II) | Ion exchange method |
| (C) | $$ \begin{aligned} \mathrm{Ca}\left(\mathrm{HCO}_3\right)_2 & +\mathrm{Ca}(\mathrm{OH})_2 \longrightarrow 2 \mathrm{CaCO}_3+2 \mathrm{H}_2 \mathrm{O} \end{aligned} $$ |
(III) | Boiling |
| (D) | $$ \begin{gathered} 2 \mathrm{NaZ}+\mathrm{Ca}^{2+}(\mathrm{aq}) \longrightarrow 2 \mathrm{Na}^{+}+\mathrm{CaZ} (\mathrm{Z}=\text { Zeolite }) \end{gathered} $$ |
(IV) | Calgon's method |
The correct answer is
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