PH3 forms bubbles when passed slowly through water but NH3 gets dissolved in water, because: 

1. NH3 forms an H-bond with water, so it is soluble but PH3 does not form an H-bond.
2. NH3 does not form an H-bond with water, so it is soluble but PH3 does form an H-bond.
3. NH3 and PHboth form H-bond with water. 
4. NH3 and PHboth do not form H-bond with water.

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The bonding present in nitrogen molecules is:
1. \(p\pi-p\pi\)
2. \(p\pi-d\pi\)
3. \(d\pi-d\pi\)
4. Only sigma bond

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NH3 forms a hydrogen bond but PH3 does not because:  

1. Phosphorus is more electronegative as compared to nitrogen.
2. Nitrogen is more electronegative as compared to phosphorus.
3. Nitrogen and phosphorous have equal electronegativity.
4. Nitrogen is more stable as compared to phosphorus.

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Match the name of process given in Column I with the name of compound given in Column II and mark the correct option.

Column I Column II
(a)  Pure nitrogen (i)  Chlorine
(b)  Haber process (ii)  Sulphuric acid
(c)  Contact process (iii)  Ammonia
(d)  Deacon's process (iv)  Sodium azide or Barium azide
 
(a) (b) (c) (d)
1. (iv) (iii) (ii) (i)
2. (i) (ii) (iii) (iv)
3. (ii) (iv) (i) (iii)
4. (iii) (iv) (ii) (i)
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 Match the formulas of oxides given in Column I with the type of oxide given in Column II and mark the correct option.

Column I Column II
A.  Pb3O4 1. Neutral oxide
B.  N2O 2. Acidic oxide
C.  Mn2O7 3. Basic oxide
D.  Bi2O3 4. Mixed oxide

Codes

A B C D
1. 1 2 3 4
2. 4 1 2 3
3. 3 2 4 1
4. 4 3 1 2
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The respective oxidation states of P in H4P2O5, H4P2O6, and H4P2O7 are: 

1. +3, +5, and +4 2. +5, +3, and +4
3. +5, +4, and +3 4. +3, +4, and +5
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A balanced chemical equation for the reaction showing catalytic oxidation of NH3 by atmospheric oxygen is:

1. 4NH3 + \(\underset{\text{From air}}{5O_2} \)   \(\xrightarrow[\text{500 K; 9 bar}]{\text{Pt / Rh gauge catalyst}}\)   4NO + 6H2O
2. 3NH4 + \(\underset{\text{From air}}{5O_2} \)  \(\xrightarrow[\text{500 K; 9 bar}]{\text{Pt / Rh gauge catalyst}}\)  3NO + 6H2O
3. 4NH3 + \(\underset{\text{From air}}{5O_2} \)  \(\xrightarrow[\text{cold}]{\text{no catalyst}}\)  4NO + 6H2O
4. 3NH4 + \(\underset{\text{From air}}{5O_2} \)  \(\xrightarrow[\text{cold}]{\text{no catalyst}}\)  3NO + 6H2O
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Nitrogen gas is liberated by the thermal decomposition of:

1. NH4NO2                                 

2. NaN3

3. NH42Cr2O7                           

4. All of the above. 

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A brown-coloured mixture of two gases is obtained by reducing 6 N nitric acid with metallic copper. This mixture on cooling condenses to a blue liquid which on freezing (-30 oC) gives a blue solid. The correct statement for the blue liquid or solid is: 

1. It is referred to as the anhydride of nitrous acid.
2. It is an acidic oxide. Hence, it dissolves in alkalies producing nitrites.
3. It can also be prepared by the action of 50 % HNO3 on arsenious oxide and then cooling to 250 K.
4. All of the above.

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The correct structure of pyrophosphoric acid is:

1. 2.
3. 4.
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