MCQ
In a chemical equilibrium $A + B$ $\rightleftharpoons$ $C + D$, when one mole each of the two reactants are mixed, $0.6 $ mole each of the products are formed. The equilibrium constant calculated is
- A$1$
- B$0.36$
- ✓$2.25$
- D$4/9$
Initial $1$ $1$ $0$ $0$
remaining at equilibrium $0.4$ $0.4$ $0.6$ $0.6$
$K = \frac{{[C]\,\,[D]}}{{[A]\,\,[B]}} = \frac{{0.6 \times 0.6}}{{0.4 \times 0.4}} = \frac{{36}}{{16}} = 2.25$.
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$MnCl _2+ K _2 S _2 O _8+ H _2 O \longrightarrow KMnO _4+ H _2 SO _4+ HCl$ (equation not balanced).
Few drops of concentrated $HCl$ were added to this solution and gently warmed. Further, oxalic acid ( $225 mg$ ) was added in portions till the colour of the permanganate ion disappeared. The quantity of $MnCl _2$ (in $mg$ ) present in the initial solution is. . . . . . . . . (Atomic weights in $g mol ^{-1}: Mn =55, Cl =35.5$ )