# 1 g of magnesium is burnt with 0.56g of oxygen in a closed vessel. <!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> The left-out reactant and its quantity are (At. weight of Mg = 24, O=16) 1. Mg, 0.16g 2. O2, 0.16g 3. Mg, 0.44g 4. O2, 0.28g

Subtopic:  Equation Based Problem |
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Percentage of Se in peroxidase anhydrase enzyme is 0.5% by weight (at. weight = 78.4), then minimum molecular weight of peroxidase anhydrase enzyme is

1. 1.568 x 10

2. 15.68

3. 2.168 x 10

4. 1.568 x 10

Subtopic:  Moles, Atoms & Electrons |
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Number of moles of Mn${\mathrm{O}}_{4}^{-}$ required to oxidise one mole of ferrous oxalate completely in acidic medium will be

1. 0.6 mole

2. 0.4 mole

3. 7.5 moles

4. 0.2 mole

Subtopic:  Equation Based Problem |
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The total number of valence electrons in 4.2g of ${\mathrm{N}}_{3}^{-}$ ion is (NA is the Avogadro's number)

1. 2.1NA

2. 4.2NA

3. 1.6NA

4. 3.2NA

Subtopic:  Moles, Atoms & Electrons |
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When 22.4L of H2(g) is mixed with 11.2L of Cl2(g) each at STP, the moles of HCl(g) formed is equal to

1. 1 mole of HCl(g)

2. 2 moles of HCl(g)

3. 0.5 mole of HCl(g)

4. 1.5 moles of  HCl(g)

Subtopic:  Moles, Atoms & Electrons |
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The mass of carbon anode consumed (giving only carbon dioxide) in the production of 270 kg of aluminium metal from bauxite by the Hall process is (at. mass of Al = 27)

1. 180 kg

2. 270 kg

3. 540 kg

4. 90 kg

Subtopic:  Equation Based Problem |
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In the Haber process, 30 L of dihydrogen and 30L of dinitrogen were taken for the reaction, which yielded only 50% of the expected product. What will be the composition of the gaseous mixture under the said conditions in the end?

1. 20L ammonia, 10L nitrogen, 30L hydrogen

2. 20L ammonia, 25L nitrogen, 15L hydrogen

3. 20L ammonia, 20L nitrogen, 20L hydrogen

4. 10L ammonia, 25L nitrogen, 15L hydrogen

Subtopic:  Limiting Reagent |
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The number of atoms in 4.25 g of NH3 is approximately

1. 4 x 1023

2. 2 x 1023

3. 1 x 1023

4. 6 x 1023

Subtopic:  Moles, Atoms & Electrons |
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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 |
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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. 201 u

2. 202 u

3. 199 u

4. 200 u

Subtopic:  Moles, Atoms & Electrons |
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