Question
Derive the Nernst equation and explain how $E_{\text {cell }}^{\circ}$ depends on concentration of ions.
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Answer
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(i) Define the order of a reaction.
(ii) Explain the effect of concentration of reactant on the rate constant.
(iii) For a first order reaction, if the rate constant at 500 K and 600 K are $0.03 s^{-1}$ and $0.06 s^{-1}$ respectively, then calculate the activation energy.
$
\left[R=8.314 JK^{-1} mol^{-1}, \log 2=0.3010\right]
$
→(ii) Explain the effect of concentration of reactant on the rate constant.
(iii) For a first order reaction, if the rate constant at 500 K and 600 K are $0.03 s^{-1}$ and $0.06 s^{-1}$ respectively, then calculate the activation energy.
$
\left[R=8.314 JK^{-1} mol^{-1}, \log 2=0.3010\right]
$
Match the complex ions given in Column I with the hybridisation and number of unpaired electrons given in Column II and assign the correct code:
Code:
→|
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Column I (Complex ion)
|
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Column II (Hybridisation, number of unpaired electrons)
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$a.$
|
$[Cr(H_2O)_6]^{3+}$
|
$1.$
|
$dsp^2, 1$
|
|
$b.$
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$[Co(CN)_4]^{2-}$
|
$2.$
|
$sp^3d^2, 5$
|
|
$c.$
|
$[Ni(NH_3)_6]^{2+}$
|
$3.$
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$d^2sp^3, 3$
|
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$d.$
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$[MnF_6]^{4-}$
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$4.$
|
$sp^3, 4$
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$5.$
|
$sp^3d^2, 2$
|
- $A (3), B (1), C (5), D (2).$
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b. HCl
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→a. $Br _2$ water
b. HCl
c. $\left( CH _3 CO \right)_2 O /$ pyridine
ii. Arrange the following in the increasing order of their boiling point:$C _2 H _5 NH _2, C _2 H _5 OH ,\left( CH _3\right)_3 N$
iii. Give a simple chemical test to distinguish between the following pair of compounds : $\left( CH _3\right)_2 NH$ and $\left( CH _3\right)_3 N$.
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(i) Physical properties
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