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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$(i)\,\, Cl^-$ can give up an electron more easily than $F^-$
$(ii) \,\,Cl^-$ is a better reducing agent than $F^-$
$(iii)\,\, Cl^-$ is smaller in size than $F^-$
$(iv)\,\, F^-$ can be oxidized more readily than $Cl^-$
$(A)$ $n=3,1=0, m=0$
$(B)$ $n=4,1=0, m=0$
$(C)$ $n =3,1=1, m =0$
$(D)$ $n=3,1=2, m=1$
$A : 1s^2\, 2s^2\, 2p^6$
$B : 1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^3$
$C : 1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^5$
$X \rightleftharpoons Y + Z - - - - - - \left( 1 \right)$
$A \rightleftharpoons 2B - - - - - - \left( 2 \right)$
are in ratio of $9 :1$. If degree of dissociation of $X$ and $A$ be equal, then total pressure at equilibrium $(1)$ and $(2)$ are in the ratio