Consider following exchange reactions - -FeH2O6-2-Cl- -FeH2O5Cl-H2O - k-106 M-1 s-1- -RuH2O6-2-Cl- -RuH2O5Cl-H2O -k-10-2M-1 s-1-Where- k- rate constant-Thus- Ru2- like other second- and third-row transition metal ions -

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Byju's Answer

Standard XII

Chemistry

Characteristics of Equilibrium Constant

Consider foll...

Question

Consider following exchange reactions :

$[F e (H_{2} O)_{6}]^{2 +} + C l^{-} \to [F e (H_{2} O)_{5} C l]^{+} + H_{2} O [k = 10^{6} M^{- 1} s^{- 1}$ ]

$[R u (H_{2} O)_{6}]^{2 +} + C l^{-} \to [R u (H_{2} O)_{5} C l]^{+} + H_{2} O [k = 10^{- 2} M^{- 1} s^{- 1}$ ]

[Where, k= rate constant]

Thus, $R u^{2 +}$ , like other second- and third-row transition metal ions :

Forms low-spin complexes.

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Low-spin

d^{6}

species are kinetically inert.

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Both of the above.

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None of the above.

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Solution

The correct option is B Both of the above.
$R u^{2 +}$ , like other second- and third-row transition metal ions forms low-spin (or spin paired) complexes.
Low-spin $d^{6}$ species are kinetically inert. In other words, they have a very small rate constant. This is exemplified by the exchange reaction
$[R u (H_{2} O)_{6}]^{2 +} + C l^{-} \to [R u (H_{2} O)_{5} C l]^{+} + H_{2} O [k = 10^{- 2} M^{- 1} s^{- 1}$ ]

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Similar questions

For the reaction:

$[C r (H_{2} O)_{6}]^{3 +} + [S C N^{⊖}] \to [C r 9 H_{2} O)_{5} N C S]^{2 +} H_{2} O$

The rate law is : $r = k [C r (H_{2} O)_{6}^{3 +} [S C N^{⊖}] .$

The value of k is $2.0 \times 10^{- 6} L m o l^{- 1} s^{- 1}$ at $14^{0}$ C and $2.2 \times 10^{- 5} L m o l^{- 1} s^{- 1}$ , at $30^{0}$ C

What is the value of $E_{a}$ ?

For the reaction:

$[C r (H_{2} O)_{6}]^{3 +} + [S C N^{⊖}] \to [C r 9 H_{2} O)_{5} N C S]^{2 +} H_{2} O$

The rate law is : $r = k [C r (H_{2} O)_{6}^{3 +} [S C N^{⊖}] .$

The value of k is $2.0 \times 10^{- 6} L m o l^{- 1} s^{- 1}$ at 14 $^{0}$ C and $2.2 \times 10^{- 5} L m o l^{- 1} s^{- 1} a t 30^{\circ} C .$ What is the value of $E_{a}$ ?

Q. The approach of the following equilibrium was observed kinetically from both directions

P t C l_{4}^{2 -} + H_{2} O ⇌ P t (H_{2} O) C l_{3}^{-} + C l^{-}

At 25°C, it is found

\frac{- d [P t C l_{4}^{2 -}]}{d t} = (3.9 \times 10^{- 5} s^{- 1)}) [P t C l_{4}^{2 -}] - (2.1 \times 10^{- 3} L m o l^{- 1} s^{- 1}) [P t (H_{2} O) C l_{3}^{-}] [C l^{-}]

Value of

K_{C}

when fourth

C l^{-}

is complexed in the reaction is:

Q. Consider the isoelectronic ions:

K^{+}, S^{2 -}, C l^{-}

and

C a^{2 +}

The radii of these ionic species follow the order:

Q. For the reaction 2A + B + C

\to A_{2} B

+ C the rate law is found to be Rate =k[A][B]

^{2}

with

k = 2 \times 10^{- 6} m o l^{- 2} L^{2} s^{- 1}

The initial rate of reaction with

[A] = 0.1 m o l L^{- 1}, [B] = 0.2 m o l L^{- 1} a n d [C] = 0.8 m o l L^{- 1}

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Consider following exchange reactions :[Fe(H2O)6]2++Cl−→[Fe(H2O)5Cl]++H2O [k=106M−1s−1][Ru(H2O)6]2++Cl−→[Ru(H2O)5Cl]++H2O [k=10−2M−1s−1][Where, k= rate constant]Thus,Ru2+, like other second- and third-row transition metal ions :