Question
Explain peroxide effect.
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Match the reactions given in Column $I$ with the suitable reagents given in Column $II.$
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Column $I ($Reactions$)$
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Column $II ($Reagents$)$
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| $(i)$ |
Benzophenone $\rightarrow$ Diphenylmethane
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$(a)$ |
$\ce{LiAlH_4}$
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| $(ii)$ |
enzaldehyde $\rightarrow 1-$Phenylethanol
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$(b)$ |
$\ce{DIBAL-H}$
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| $(iii)$ |
Cyclohexanone $\rightarrow$ Cyclohexanol
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$(c)$ |
$\ce{Zn(Hg)/Conc. HCl}$
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| $(iv)$ |
Phenyl benzoate $\rightarrow$ Benzaldehyde
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$(d)$ |
$\ce{CH_3MgBr}$
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In a pseudo first order hydrolysis of ester in water, the following results were obtained:
→| $t/s$ | $0$ | $30$ | $60$ | $90$ |
| $[$Ester$]/mol \ L^{-1}$ | $0.55$ | $0.31$ | $0.17$ | $0.085$ |
- Calculate the average rate of reaction between the time interval $30$ to $60$ seconds.
- Calculate the pseudo first order rate constant for the hydrolysis of ester.
Draw the tetrahedral intermediate formed by nucleophilic attack on carbonyl carbon in nucleophilic addition reaction.
Explain the preparation of aldehydes and ketones by dehydrogenation of alcohols with suitable examples.
Why are $Mn^{2+}$ compounds more stable than $Fe^{2+}$ towards oxidation to their $+3$ state?
→Why is the reactivity of all the three classes of alcohols with conc. $\ce{HCl}$ and $\ce{ZnCl_2} ($Lucas reagent$)$ different?
→The molar conductivity of a $1.5M$ solution of an electrolyte is found to be $138.9 \ \ce{Scm^{2 }mol^{–1}}.$ Calculate the conductivity of this solution.
→Write the name of the cell which is generally used in transistors. Write the reactions taking place at the anode and the cathode of this cell.
If a current of $0.5$ ampere flows through a metallic wire for $2$ hours, then how many electrons would flow through the wire?
→Two half-reactions of an electrochemical cell are given below:
$MnO_4^- (aq) + 8 H^+ (aq) + 5e^– \rightarrow Mn^{2+} (aq) + 4H_2O (l), E^\circ = +1.51 V,$
$Sn^{2+} (aq) \rightarrow Sn^{4+} (aq) + 2e^–, E^\circ= +0.15 V.$
Construct the redox reaction equation from the two half-reactions and calculate the cell potential from the standard potentials and predict if the reaction is reactant or product favoured.
→$MnO_4^- (aq) + 8 H^+ (aq) + 5e^– \rightarrow Mn^{2+} (aq) + 4H_2O (l), E^\circ = +1.51 V,$
$Sn^{2+} (aq) \rightarrow Sn^{4+} (aq) + 2e^–, E^\circ= +0.15 V.$
Construct the redox reaction equation from the two half-reactions and calculate the cell potential from the standard potentials and predict if the reaction is reactant or product favoured.