The total number of electrons present in 1.6 gm. of methane is [IIT 1976; Roorkee 1985; CPMT 1987, 92]

(1) 6.02 × 1023

(2) 6.02 × 1022

(3) 6.02 × 1021

(4) 4.02 × 1020

Subtopic:  Moles, Atoms & Electrons |
 66%
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KClO3 on heating decomposes to KCl and O2. The volume of O2 at STP liberated by 0.1 mole KClO3 is

1. 4.36 L

2. 3.36 L

3. 2.36 L

4. None of these

Subtopic:  Equation Based Problem |
 73%
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At S.T.P. the density of CCl4 vapour in g/L will be nearest to [CBSE PMT 1988]

(1) 6.84

(2) 3.42

(3) 10.26

(4) 4.57

Subtopic:  Moles, Atoms & Electrons |
 68%
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4.4 g of an unknown gas occupies 2.24 litres of volume at NTP. The gas may be: 

1. Carbon dioxide 2. Carbon monoxide
3. Oxygen 4. Sulphur dioxide
Subtopic:  Moles, Atoms & Electrons |
 87%
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The number of gram molecules of oxygen in 6.02 × 1024 CO molecules are:

1. 10 g molecules

2. 5 g molecules

3. 1 g molecules

4. 0.5 g molecules

Subtopic:  Moles, Atoms & Electrons |
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The mass of carbon present in 0.5 mole of K4[Fe(CN)6] is:

1. 1.8 g

2. 18 g

3.  3.6 g

4.  36 g

Subtopic:  Moles, Atoms & Electrons |
 72%
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The number of moles of BaCO3 which contains 1.5 moles of oxygen atoms is:

1. 0.5

2. 1

3. 3

4. 6.02 ×1023

Subtopic:  Equation Based Problem |
 74%
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The oxide of metal contains 40% by mass of oxygen. The percentage of chlorine in the chloride of the metal is

1. 84.7

2. 74.7

3. 64.7

4. 44.7

Subtopic:  Millimole/Equivalent Concept |
 55%
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The empirical formula of an organic compound containing carbon and hydrogen is CH2. The mass of one litre of this organic gas at STP  is exactly equal to that of one litre of N2 at STP. Therefore, the molecular formula of the organic gas is:

1. C2H4

2. C3H6

3. C6H12

4. C4H8

Subtopic:  Moles, Atoms & Electrons | Empirical & Molecular Formula |
 77%
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A sample of pure compound is found to have Na = 0.0887 mole, O = 0.132 mole, C = 2.65 × 1022 atoms.

The empirical formula of the compound is 

(1) Na2CO3

(2) Na3O2C5

(3) Na0.088700.132C2.65×1022

(4) NaCO

Subtopic:  Empirical & Molecular Formula |
 62%
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