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# What is the approximate number of atoms present in 4.25 grams of NH3? 1. 4 x 1023  2. 2 x 1023  3. 1 x 1023  4. 6 x 1023

Subtopic:  Moles, Atoms & Electrons |
57%
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In the reaction, 4NH3(g)+ 5O2(g) $\to$4NO(g) +6H2O(l)

When 1 mole of ammonia and 1 mole of O2  reacts to completion, then:

 1 1.0 mole of H2O is produced. 2 1.0 mole of NO will be produced. 3 All the oxygen will be consumed. 4 All the ammonia will be consumed.

Subtopic:  Equation Based Problem |
69%
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An element X has the following isotopic composition,

200X : 90%, 199X : 8.0%, 202X : 2.0%

The weighted average atomic mass of the naturally occurring element X is closest to:

 1 205 u 2 220 u 3 196 u 4 200 u
Subtopic:  Moles, Atoms & Electrons |
64%
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0.24g of a volatile gas, upon vaporisation, gives 45 mL vapour at NTP. What will be the vapour density of the substance?

(Density of H2 = 0.089)

1. 95.93

2. 59.93

3. 95.39

4. 5.993

Subtopic:  Moles, Atoms & Electrons |
62%
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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
Subtopic:  Empirical & Molecular Formula |
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12 g of Mg (atomic mass = 24) will react completely with an acid to yield:

1. One mole of H

2. A half mole of H2

3. One mole of O2

4. None of the above

Subtopic:  Equation Based Problem |
69%
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The molality of a 15% (w/vol.) solution of H2SO4 of density 1.1g/cm3 is-

1. 1.2

2. 1.4

3. 1.8

4. 1.6

Subtopic:  Concentration Based Problem |
51%
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Which mode of expressing concentration is independent of temperature?

1. Molality

2. Percent by mass

3. Mole fraction

4. All of the above

Subtopic:  Concentration Based Problem |
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The product of atomic mass and specific heat of metal is approximately 6.4. This was given by:

1. Dalton's law

3. Newton's law

4. Dulong Petit's law

Subtopic:  Introduction |
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A metal M forms a compound M2HPO4. The formula of the metal sulphate is:

1. M2SO4

2. MSO4

3. M(SO4${\right)}_{2}$

4. M2(SO4)3

Subtopic:  Empirical & Molecular Formula |
62%
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