Question
Expian the basic properties of amines.

Answer

SELF

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Describe the reactions of carboxylic acids in which C-OH bond is broken.
Match the terms given in Column I with expressions given in Column II.
  Column I
  Column II
i. Mass percentage
a. $\frac{\text{Number of moles of the solute component}}{\text{Volume of solution in litres}}$
ii. Volume percentage
b. $\frac{\text{Number of moles of a component}}{\text{Total number of moles of all the components}}$
iii. Mole fraction
c. $\frac{\text{Volume of the solute component in solution}}{\text{Total volume of solution}}\times100$
iv. Molality
d. $\frac{\text{Mass of the solute component in solution}}{\text{Total mass of the solution}}\times100$
v. Molarity
e. $\frac{\text{Number of moles of the solute components}}{\text{Mass of solvent in kilograms}}$
Explain the elimination reaction of haloalkanes.
Explain the reaction of various ethers with hydrogen halide with the mechanism.
  1. Give reasons for the following:
  1. Mn3+ is a good oxidizing agent.
  2. Eo m2+/M values are not regular for first row transition metals. (3d series)
  3. Although ‘F’ is more electronegative then ‘O’, the highest Mn fluoride is Mnf4, whereas the highest oxide is Mn2O7.
  1. Complete the following equations:

$\text{2CrO}_{4}^{2}+\text{2H}^{+}\rightarrow$

$\text{KMnO}_{4}\xrightarrow{heat}$

  1. Write the steps involved in the preparation of: 
  1. K2Cr2O7 from Na2CrO4.
  2. KMnO4 from  K2MnO4.
  3. Calomel from corrosive sublimate.
  1. What is meant by lanthanoid contraction? What effect does it have on the chemistry of the elements which follow lanthanoids?
 Match the compounds given in Column I with the oxidation state of cobalt present in it (given in Column II) and assign the correct code.

 
Column I (Compound)
 
Column II (Oxidation state of Co)
a.
[Co(NCS)(NH3)5](SO3)
1.
+4
b.
[Co(NH3)4Cl2]SO4
2.
0
c.
Na4[Co(S2O3)3]
3.
+1
d.
[Co2(CO)8]
4.
+2
 
 
5.
+3

Code:

  1. A (1), B (2), C (4), D (5).
  2. A (4), B (3), C (2), D (1).
  3. A (5), B (1), C (4), D (2).
  4. A (4), B (1), C (2), D (3).
A voltaic cell is set up at 25°C with the followinng half-cell:
Al | Al3+ (0.001M) and Ni | Ni2+ (0.50M)
Calculate the cell voltage $\text{E}^{\circ}_{\text{Ni}^{2+}/\text{Ni}}\Big[=-0.25\text{V,E}^{\circ}_{\text{Al}^{3+}/\text{Al}}=-1.66\text{V}\Big]$
Match the terms given in Column I with the units given in Column II.

 
Column I

 

Column II

i.

$\wedge_{\text{m}}$

a.

Intensive property.

ii.

$\text{E}^{\ominus}_{\text{Cell}}$

b.

Depends on number of ions/volume.

iii.

$\text{K}$

c.

Extensive property.

iv.

$\Delta_{\text{r}}\text{G}_{\text{Cell}}$

d.

Increases with dilution.

Match the items of Column I and Column II on the basis of data given below:
$\text{E}^{\ominus}_{\text{F}_2/\text{F}^-}=2.87\text{V},\text{ E}^{\ominus}_{\text{Li}^+/\text{Li}}=-3.5\text{V},\text {E}^{\ominus}_{\text{Au}^{3+}/\text{Au}}=1.4\text{V},\text{ E}^{\ominus}_{ \text{Br}_2/\text{Br}^-}=1.09\text{V}$
 
Column I
 
Column II
i.
F2
a.
Metal is the strongest reducing agent.
ii.
Li
b.
Metal ion which is the weakest oxidising agent.
iii.
Au3+
c.
Non metal which is the best oxidising agent.
iv.
Br-
d.
Unreactive metal.
v.
Au
e.
Anion that can be oxidised by Au3+
vi.
Li+
f.
Anion which is the weakest reducing agent.
vii.
F-
g.
Metal ion which is an oxidising agent.