The empirical formula and molecular mass of a compound are CH2O and 180 g, respectively. The molecular formula of the compound is:
1. C9H18O9
2. CH2O
3. C6H12O6
4. C2H4O2

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The molar mass of naturally occurring Argon isotopes is: 

Isotope Isotopic molar mass Abundance
36-Ar  35.96755 g mol–1 0.337%
38-Ar  37.96272 g mol–1  0.063%
40-Ar  39.9624 g mol–1  99.600%
 
1. 49.99947 g mol-1  2. 39.99947 g mol-1  
3. 35.59947 g mol-1   4. 45.59947 g mol-1  
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On complete combustion, 44 g of a sample of a compound gives 88 g CO2 and 36 g of H2O. The molecular formula of the compound may be:

1.  C4H6 

2.  C2H6O 

3.  C2H4O

4.  C3H6O

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An organic compound contains carbon, hydrogen, and oxygen. Its elemental analysis gave C, 38.71%, and H, 9.67%. The empirical formula of the compound would be:

1. CH3O 2. CH2O
3. CHO 4. CH4O
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Assertion (A): The empirical mass of ethene is half of its molecular mass.
Reason (R): The empirical formula represents the simplest whole-number ratio of the various atoms present in a compound.
 
1. Both (A) and (R) are True and (R) is the correct explanation of (A).
2. Both (A) and (R) are True but (R) is not the correct explanation of (A).
3. (A) is True but (R) is False.
4. (A) is False but (R) is True.
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In an iron oxide, the mass percent of iron and oxygen are 69.9 and 30.1, respectively. The empirical formula of the oxide of iron will be:

1. Fe3O2

2. Fe2O2

3. Fe2O3

4. Fe3O4

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 If 2.74 g of the metal oxide contains 1.53 g of metal, then the empirical formula of vanadium oxide is:

(Atomic Mass of V = 52)

1. V2O3

2. VO

3. V2O5

4. V2O7

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The hydrated salt, Na2SO4.nH2O, undergoes a 55% loss in mass on heating and becomes anhydrous. The value of n will be:

1. 5 2. 3
3. 7 4. 10
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